Methods of sequestering CO2

ABSTRACT

Methods of sequestering carbon dioxide (CO2) are provided. Aspects of the methods include precipitating a storage stable carbon dioxide sequestering product from an alkaline-earth-metal-containing water and then disposing of the product, e.g., by placing the product in a disposal location or using the product as a component of a manufactured composition. Also provided are systems for practicing methods of the invention.

CROSS-REFERENCE TO RELATED APPLICATIONS

Pursuant to 35 U.S.C. §119 (e), this application claims priority to thefiling dates of: U.S. Provisional Patent Application Ser. No. 61/017,405filed on Dec. 28, 2007; U.S. Provisional Patent Application Ser. No.61/057,173 filed on May 29, 2008; U.S. Provisional Patent Application61/073,319 filed on Jun. 17, 2008; U.S. Provisional Patent Application61/082,766 filed on Jul. 22, 2008; U.S. Provisional Patent ApplicationSer. No. 61/088,340 filed on Aug. 12, 2008; U.S. Provisional PatentApplication Ser. No. 61/088,347 filed on Aug. 13, 2008; U.S. ProvisionalPatent Application Ser. No. 61/101,626 filed on Sep. 30, 2008; and U.S.Provisional Patent Application No. 61/121,872 filed on Dec. 11, 2008;and Pursuant to 35 U.S.C. §120, this application claims priority to thefiling dates of PCT Application No. PCT/US08/88242 entitled “Low-EnergyElectrochemical Hydroxide System and Method,” filed on Dec. 23, 2008,and PCT Application No. PCT/US08/88246 entitled “Low-EnergyElectrochemical Proton Transfer System and Method,” filed on Dec. 23,2008; the disclosures of which applications are herein incorporated byreference.

INTRODUCTION

Carbon dioxide (CO₂) emissions have been identified as a majorcontributor to the phenomenon of global warming and ocean acidification.CO₂ is a by-product of combustion and it creates operational, economic,and environmental problems. It is expected that elevated atmosphericconcentrations of CO₂ and other greenhouse gases will facilitate greaterstorage of heat within the atmosphere leading to enhanced surfacetemperatures and rapid climate change. CO₂ has also been interactingwith the oceans driving down the pH toward 8.0 from 8.2. CO₂ monitoringhas shown atmospheric CO₂ has risen from approximately 280 ppm in the1950s to approximately 380 pmm today, and is expect to exceed 400 ppm inthe next decade. The impact of climate change will likely beeconomically expensive and environmentally hazardous. Reducing potentialrisks of climate change will require sequestration of atmospheric CO₂.

Many types of industrial plants (such as cement refineries, steel millsand power plants) combust various carbon-based fuels, such as fossilfuels and syngases. Fossil fuels that are employed include coal, naturalgas, oil, used tires, municipal waste, petroleum coke and biofuels.Fuels are also derived from tar sands, oil shale, coal liquids, and coalgasification and biofuels that are made via syngas. CO₂ concentrationsin the exhaust gases of various fuels vary from a few % to nearly pureCO₂. Cement plants are a major source of CO₂ emissions, from both theburning of fossil fuels and the CO₂ released from calcination whichchanges limestone, shale and other ingredients to Portland cement.Similarly, power plants which utilize combustion of carbon-based fuelsto generate electricity are also a major source of CO₂ emissions. Manyindustrial plants also produce several other pollutants including NOx,SOx, VOCx, particulates and mercury, in addition to wasted heat.Furthermore, many industrial plants can produce materials such as cementkiln dust from a cement production plant or ash from coal-fired powerplants, that must sometimes be disposed in hazardous material landfillsites.

Methods proposed to separate CO₂ from flue gas, contain it and store CO₂include storage in geological formations, injection into the deep-ocean,and uptake by phytoplankton via fertilization of the ocean. The limitedcapacity and duration, expense, and environmental outcomes of thesemethods are largely unresolved and may prohibit their utility.

SUMMARY

Methods of sequestering carbon dioxide (CO₂) are provided. Aspects ofthe methods include precipitating a storage stable carbon dioxidesequestering product from an alkaline-earth-metal-containing water andthen disposing of the product, e.g., by placing the product in adisposal location or using the product as a component of a manufactureditem, such as a building material. Also provided are systems forpracticing methods of the invention.

BRIEF DESCRIPTION OF THE FIGURES

FIG. 1 provides a schematic diagram of a CO₂ sequestration methodaccording to one embodiment of the invention.

FIG. 2 provides a schematic diagram of a CO₂ sequestration systemaccording to another embodiment of the invention.

FIG. 3 provides a schematic diagram of power plant that is integratedwith a CO₂ sequestration system according to an embodiment of theinvention.

FIG. 4 provides a schematic diagram of a portland cement plant.

FIG. 5 provides a schematic diagram of a cement plant co-located with aprecipitation plant according to one embodiment of the invention

FIG. 6 provides a schematic of a cement plant which does not require amined limestone feedstock according to one embodiment of the invention

FIG. 7A provides a diagram of one embodiment of a bi-electrode apparatusfor removing protons form solutions electrochemically.

FIG. 7B provides a diagram of one embodiment of a bi-electrode apparatusfor removing protons form solutions electrochemically.

FIG. 8 provides a diagram of one embodiment of a low-voltage apparatusfor producing hydroxide electrochemically.

FIG. 9 provides a diagram of another embodiment of a low-voltageapparatus for producing hydroxide electrochemically.

FIG. 10 provides a diagram of another embodiment of a low-voltageapparatus for producing hydroxide electrochemically.

FIG. 11 provides a schematic of a system according to one embodiment ofthe invention.

FIGS. 12A, 12B and 12C provide schematics of a system according to oneembodiment of the invention.

FIGS. 13A and 13B provide pictures of precipitate of the invention.

FIG. 14 provides a picture of amorphous precipitate of the invention.

FIG. 15 provides graphical results of a CO₂ absorption experimentreported in the Experimental Section, below.

RELEVANT CHEMICAL REACTIONS

The methods and systems of the invention utilize processes summarized bythe following chemical reactions:

-   -   (1) Combustion of a carbon-containing fuel source in liquid,        gas, or solid phase forms gaseous carbon dioxide:        C+O₂(g)→CO₂(g)    -   (2) Contacting the source of carbon dioxide with a water source        solvates the carbon dioxide to give an aqueous solution of        carbon dioxide:        CO₂(g)→CO₂(aq)    -   (3) Carbon dioxide dissolved in water establishes equilibrium        with aqueous carbonic acid:

-   -   (4) Carbonic acid is a weak acid which dissociates in two steps,        where the equilibrium balance is determined in part by the pH of        the solution, with, generally, pHs below 8-9 favoring        bicarbonate formation and pHs above 9-10 favoring carbonate        formation. In the second step, a hydroxide source may be added        to increase alkalinity:

-   -   Reaction of elemental metal cations from Group IIA with the        carbonate anion forms a metal carbonate precipitate:

wherein X is any element or combination of elements that can chemicallybond with a carbonate group or its multiple and m and n arestoichiometric positive integers.

DETAILED DESCRIPTION

Methods of sequestering carbon dioxide (CO₂) are provided. Aspects ofthe methods include precipitating a storage stable carbon dioxidesequestering product from an alkaline-earth-metal-containing water andthen disposing of the product, e.g., by placing the product in adisposal location or using the product as a component of a manufactureditem, such as a building material. Also provided are systems forpracticing methods of the invention.

Before the present invention is described in greater detail, it is to beunderstood that this invention is not limited to particular embodimentsdescribed, as such may, of course, vary. It is also to be understoodthat the terminology used herein is for the purpose of describingparticular embodiments only, and is not intended to be limiting, sincethe scope of the present invention will be limited only by the appendedclaims.

Where a range of values is provided, it is understood that eachintervening value, to the tenth of the unit of the lower limit unlessthe context clearly dictates otherwise, between the upper and lowerlimit of that range and any other stated or intervening value in thatstated range, is encompassed within the invention. The upper and lowerlimits of these smaller ranges may independently be included in thesmaller ranges and are also encompassed within the invention, subject toany specifically excluded limit in the stated range. Where the statedrange includes one or both of the limits, ranges excluding either orboth of those included limits are also included in the invention.

Certain ranges are presented herein with numerical values being precededby the term “about.” The term “about” is used herein to provide literalsupport for the exact number that it precedes, as well as a number thatis near to or approximately the number that the term precedes. Indetermining whether a number is near to or approximately a specificallyrecited number, the near or approximating unrecited number may be anumber which, in the context in which it is presented, provides thesubstantial equivalent of the specifically recited number.

Unless defined otherwise, all technical and scientific terms used hereinhave the same meaning as commonly understood by one of ordinary skill inthe art to which this invention belongs. Although any methods andmaterials similar or equivalent to those described herein can also beused in the practice or testing of the present invention, representativeillustrative methods and materials are now described.

All publications and patents cited in this specification are hereinincorporated by reference as if each individual publication or patentwere specifically and individually indicated to be incorporated byreference and are incorporated herein by reference to disclose anddescribe the methods and/or materials in connection with which thepublications are cited. The citation of any publication is for itsdisclosure prior to the filing date and should not be construed as anadmission that the present invention is not entitled to antedate suchpublication by virtue of prior invention. Further, the dates ofpublication provided may be different from the actual publication dateswhich may need to be independently confirmed.

It is noted that, as used herein and in the appended claims, thesingular forms “a”, “an”, and “the” include plural referents unless thecontext clearly dictates otherwise. It is further noted that the claimsmay be drafted to exclude any optional element. As such, this statementis intended to serve as antecedent basis for use of such exclusiveterminology as “solely,” “only” and the like in connection with therecitation of claim elements, or use of a “negative” limitation.

As will be apparent to those of skill in the art upon reading thisdisclosure, each of the individual embodiments described and illustratedherein has discrete components and features which may be readilyseparated from or combined with the features of any of the other severalembodiments without departing from the scope or spirit of the presentinvention. Any recited method can be carried out in the order of eventsrecited or in any other order which is logically possible.

In further describing the subject invention, the methods of CO₂sequestration according to embodiments of the invention are describedfirst in greater detail. Next systems that find use in practicingvarious embodiments of the methods of the invention are reviewed.

Methods of CO₂ Sequestration

As reviewed above, the invention provides methods of CO₂ sequestration.By “CO₂ sequestration” is meant the removal or segregation of an amountof CO₂ from an environment, such as the Earth's atmosphere or a gaseouswaste stream produced by an industrial plant, so that some or all of theCO₂ is no longer present in the environment from which it has beenremoved. CO₂ sequestering methods of the invention sequester CO₂producing a storage stable carbon dioxide sequestering product from anamount of CO₂, such that the CO₂ from which the product is produced isthen sequestered in that product. The storage stable CO₂ sequesteringproduct is a storage stable composition that incorporates an amount ofCO₂ into a storage stable form, such as an above-ground storage orunderwater storage stable form, so that the CO₂ is no longer present as,or available to be, a gas in the atmosphere. As such, sequestering ofCO₂ according to methods of the invention results in prevention of CO₂gas from entering the atmosphere and allows for long term storage of CO₂in a manner such that CO₂ does not become part of the atmosphere.

Embodiments of methods of the invention are negative carbon footprintmethods. By “negative carbon footprint” is meant that the amount byweight of CO₂ that is sequestered (e.g., through conversion of CO₂ tocarbonate) by practice of the methods is greater that the amount of CO₂that is generated (e.g., through power production, base production, etc)to practice the methods. In some instances, the amount by weight of CO₂that is sequestered by practicing the methods exceeds the amount byweight of CO₂ that is generated in practicing the methods by 1 to 100%,such as 5 to 100%, including 10 to 95%, 10 to 90%, 10 to 80%, 10 to 70%,10 to 60%, 10 to 50%, 10 to 40%, 10 to 30%, 10 to 20%, 20 to 95%, 20 to90%, 20 to 80%, 20 to 70%, 20 to 60%, 20 to 50%, 20 to 40%, 20 to 30%,30 to 95%, 30 to 90%, 30 to 80%, 30 to 70%, 30 to 60%, 30 to 50%, 30 to40%, 40 to 95%, 40 to 90%, 40 to 80%, 40 to 70%, 40 to 60%, 40 to 50%,50 to 95%, 50 to 90%, 50 to 80%, 50 to 70%, 50 to 60%, 60 to 95%, 60 to90%, 60 to 80%, 60 to 70%, 70 to 95%, 70 to 90%, 70 to 80%, 80 to 95%,80 to 90%, and 90 to 95%. In some instances, the amount by weight of CO₂that is sequestered by practicing the methods exceeds the amount byweight of CO₂ that is generated in practicing the methods by 5% or more,by 10% or more, by 15% or more, by 20% or more, by 30% or more, by 40%or more, by 50% or more, by 60% or more, by 70% or more, by 80% or more,by 90% or more, by 95% or more.

As summarized above, the methods of invention produce a precipitatedstorage stable carbon dioxide sequestering product, such that the carbondioxide is sequestered in a “storage stable form”. By “storage stableform” is meant a form of matter that can be stored, for example aboveground or underwater, under exposed conditions (for example, open to theatmosphere, underwater environment, etc.), without significant, if any,degradation for extended durations, e.g., 1 year or longer, 5 years orlonger, 10 years or longer, 25 years or longer, 50 years or longer, 100years or longer, 250 years or longer, 1000 years or longer, 10,000 yearsor longer, 1,000,000 years or longer, or 100,000,000 years or longer, or1,000,000,000 years or longer. As the storage stable form undergoeslittle if any degradation while stored above ground under normal rainwater pH, the amount of degradation if any as measured in terms of CO₂gas release from the product will not exceed 5%/year, and in certainembodiments will not exceed 1%/year or 0.001% per year. The above-groundstorage stable forms are storage stable under a variety of differentenvironment conditions, e.g., from temperatures ranging from −100° to600° C., humidity ranging from 0% to 100% where the conditions may becalm, windy or stormy. In some instances, the storage stable product isemployed as a component of a manufactured item, such as a buildingmaterial, e.g., component of a cement or concrete. In these embodiments,the product is still a storage stable CO₂ sequestering product, as useof the product in the manufactured item (such as building material) doesnot result in release of CO₂ from the product. In certain embodiments,the carbonate compounds of the precipitate when combined with portlandcement may dissolve and combine with compounds of the portland cement,without releasing CO₂.

The amount of carbon present in storage stable carbon dioxidesequestering products produced by methods of the invention may vary. Insome instances, the amount of carbon that is present in the precipitatedproduct (as determined by using protocols described in greater detailbelow, such as isotopic analysis, e.g., ¹³C isotopic analysis) in theproduct ranges from 1% to 15% (w/w), such as 5 to 15% (w/w), andincluding 5 to 14% (w/w), 5 to 13% (w/w), 6 to 14% (w/w), 6 to 12%(w/w), and 7 to 12% (w/w). Where the method employed to produce theprecipitated product includes contacting a water with a source of CO₂(for example as described in greater detail below), a substantial amountof the carbon may be carbon that originated (as determined by protocolsdescribed in greater detail below) in the source of CO₂. By substantialamount is meant that 10 to 100%, such as 50 to 100% and including 90 to100% of the carbon present in the storage stable carbon dioxidesequestering product is from the carbon dioxide source (such as a carbondioxide containing gaseous stream). In some instances, the amount ofcarbon present in the product that is traceable to the carbon dioxidesource is 50% or more, 60% or more, 70% or more, 80% or more, 90% ormore, 95% or more, 99% or more, including 100%.

In certain embodiments, the CO₂ sequestering product can store about 50tons or more of CO₂, such as about 100 tons or more of CO₂, including150 tons or more of CO₂, for instance about 200 tons or more of CO₂,such as about 250 tons or more of CO₂, including about 300 tons or moreof CO₂, such as about 350 tons or more of CO₂, including 400 tons ormore of CO₂, for instance about 450 tons or more of CO₂, such as about500 tons or more of CO₂, including about 550 tons or more of CO₂, suchas about 600 tons or more of CO₂, including 650 tons or more of CO₂, forinstance about 700 tons or more of CO₂, for every 1000 tons of CO₂sequestering product, e.g., a material to be used in the builtenvironment such as cement or aggregate, produced. Thus, in certainembodiments, the CO₂ sequestering product comprises about 5% or more ofCO₂, such as about 10% or more of CO₂, including about 25% or more ofCO₂, for instance about 50% or more of CO₂, such as about 75% or more ofCO₂, including about 90% or more of CO₂.

Storage stable CO₂ sequestering products produced by methods of theinvention may include carbonate compounds that, upon combination withfresh water, dissolve and produce different minerals that are morestable in fresh water than compounds of the initial precipitate productcomposition. (Although the compounds of the initial precipitate productcomposition may dissolve upon combination with freshwater and thenproduce different components, CO₂ gas is not liberated in significantamounts, or in some cases at all, in any such reaction). The compoundsof the initial precipitate product composition may be ones that are morestable in salt water than they are in freshwater, such that they may beviewed as saltwater metastable compounds. The amount of carbonate in theproduct, as determined by coulometry using the protocol described incoulometric titration, is 40% or higher, such as 70% or higher,including 80% or higher.

The storage stable precipitated product may include one or moredifferent carbonate compounds, such as two or more different carbonatecompounds, e.g., three or more different carbonate compounds, five ormore different carbonate compounds, etc., including non-distinct,amorphous carbonate compounds. Carbonate compounds of precipitatedproducts of the invention may be compounds having a molecularformulation X_(m)(CO₃)_(n) where X is any element or combination ofelements that can chemically bond with a carbonate group or itsmultiple, wherein X is in certain embodiments an alkaline earth metal(elements found in column IIA of the periodic table of elements) and notan alkali metal (elements found in column IA of the periodic table ofelements); wherein m and n are stoichiometric positive integers. Thesecarbonate compounds may have a molecular formula of X_(m)(CO₃)_(n).H₂O,where there are one or more structural waters in the molecular formula.

The carbonate compounds may be amorphous or crystalline. The particularmineral profile, i.e., the identity of the different types of differentcarbonate minerals and the amounts of each, in the carbonate compoundcomposition may vary and will be dependent on the particular nature ofthe water source from which it is derived, as well as the particularconditions employed to derive it.

As indicated above, in some embodiments of the invention, the carbonatecompounds of the compositions are metastable carbonate compounds thatare more stable in saltwater than in freshwater, such that upon contactwith fresh water of any pH they dissolve and reprecipitate into otherfresh water stable minerals. In certain embodiments, the carbonatecompounds are present as small particles, e.g., with particle sizesranging from 0.1 microns to 100 microns, e.g., 1 to 100 microns, or 10to 100 microns, or 50 to 100 microns, in some embodiments 0.5 to 10microns, as determined by scanning electron microscopy. In someembodiments, the particle sizes exhibit a bimodal or multi-modaldistribution. In certain embodiments, the particles have a high surfaceare, e.g., ranging from 0.5 to 100 m²/gm, 0.5 to 50 m²/gm, such as from0.5 to 2.0 m²/gm, as determined by Brauner, Emmit, & Teller (BET)Surface Area Analysis. In some embodiments, the CO₂ sequesteringproducts produced by methods of the invention may include rod-shapedcrystals and amorphous solids. The rod-shaped crystals may vary instructure, and in certain embodiments have length to diameter ratioranging from 500 to 1, such as 10 to 1. In certain embodiments, thelength of the crystals ranges from 0.5 μm to 500 μm, such as from 5 μmto 100 μm. In yet other embodiments, substantially completely amorphoussolids are produced.

The carbonate compounds of the precipitated products may include anumber of different cations, such as but not limited to: calcium,magnesium, sodium, potassium, sulfur, boron, silicon, strontium, andcombinations thereof. Of interest are carbonate compounds of divalentmetal cations, such as calcium and magnesium carbonate compounds.Specific carbonate compounds of interest include, but are not limitedto: calcium carbonate minerals, magnesium carbonate minerals and calciummagnesium carbonate minerals. Calcium carbonate minerals of interestinclude, but are not limited to: calcite (CaCO₃), aragonite (CaCO₃),vaterite (CaCO₃), ikaite (CaCO₃.6H₂O), and amorphous calcium carbonate(CaCO₃.nH₂O). Magnesium carbonate minerals of interest include, but arenot limited to magnesite (MgCO₃), barringtonite (Mg CO₃.2H₂O),nesquehonite (Mg CO₃.3H₂O), lanfordite (MgCO₃.5H₂O), hydromagnisite, andamorphous magnesium carbonate (MgCO₃.nH₂O). Calcium magnesium carbonateminerals of interest include, but are not limited to dolomite (CaMgCO₃),huntitte (CaMg(CO₃)₄) and sergeevite (Ca₂Mg₁₁(CO₃)₁₃.H₂O). The carboncompounds of the product may include one or more waters of hydration, ormay be anhydrous.

In some instances, the amount by weight of magnesium carbonate compoundsin the precipitate exceeds the amount by weight of calcium carbonatecompounds in the precipitate. For example, the amount by weight ofmagnesium carbonate compounds in the precipitate may exceed the amountby weight calcium carbonate compounds in the precipitate by 5% or more,such as 10% or more, 15% or more, 20% or more, 25% or more, 30% or more.In some instances, the weight ratio of magnesium carbonate compounds tocalcium carbonate compounds in the precipitate ranges from 1.5-5 to 1,such as 2-4 to 1 including 2-3 to 1.

In some instances, the precipitated product may include hydroxides, suchas divalent metal ion hydroxides, e.g., calcium and/or magnesiumhydroxides. The principal calcium hydroxide mineral of interest isportlandite Ca(OH)₂, and amorphous hydrated analogs thereof. Theprincipal magnesium hydroxide mineral of interest is brucite Mg(OH)₂,and amorphous hydrated analogs thereof.

As the precipitated products are derived from analkaline-earth-metal-ion-containing water source, they will include oneor more components that are present in the water source from which theyare precipitated and identify the compositions that come from the watersource, where these identifying components and the amounts thereof arecollectively referred to herein as a water source identifier. Forexample, if the water source is sea water, identifying compounds thatmay be present in carbonate compound compositions include, but are notlimited to: chloride, sodium, sulfur, potassium, bromide, silicon,strontium and the like. Any such source-identifying or “marker” elementsare generally present in small amounts, e.g., in amounts of 20,000 ppmor less, such as amounts of 2000 ppm or less. In certain embodiments,the “marker” compound is strontium, which may be present in theprecipitate incorporated into the aragonite lattice, and make up 10,000ppm or less, ranging in certain embodiments from 3 to 10,000 ppm, suchas from 5 to 5000 ppm, including 5 to 1000 ppm, e.g., 5 to 500 ppm,including 5 to 100 ppm. Another “marker” compound of interest ismagnesium, which may be present in amounts of up to 20% molesubstitution for calcium in carbonate compounds. The water sourceidentifier of the compositions may vary depending on the particularwater source, e.g., saltwater employed to produce the water-derivedcarbonate composition. In certain embodiments, the calcium carbonatecontent of the precipitate is 25% w/w or higher, such as 40% w/w orhigher, and including 50% w/w or higher, e.g., 60% w/w. The carbonatecompound composition has, in certain embodiments, a calcium/magnesiumratio that is influenced by, and therefore reflects, the water sourcefrom which it has been precipitated. In certain embodiments, thecalcium/magnesium molar ratio ranges from 10/1 to 1/5 Ca/Mg, such as 5/1to 1/3 Ca/Mg. In certain embodiments, the carbonate composition ischaracterized by having a water source identifying carbonate tohydroxide compound ratio, where in certain embodiments this ratio rangesfrom 100 to 1, such as 10 to 1 and including 1 to 1.

In methods of the invention, an alkaline-earth-metal-ion-containingwater is subjected to carbonate compound precipitation conditions toproduce the precipitated storage stable carbon dioxide sequesteringproduct. The alkaline-earth-metal-ion-containing water may varydepending on the particular method of sequestration that is to beperformed. One type of water of interest is saltwater. The term“saltwater” is employed in its conventional sense to refer a number ofdifferent types of aqueous fluids other than fresh water, where the term“saltwater” includes brackish water, sea water and brine (includingman-made brines, such as geothermal plant wastewaters, desalinationwaste waters, etc, as well as natural brines such as surface brinesfound in bodies of water on the surface of the earth and deep brines,found underneath the earth), as well as other salines having a salinitythat is greater than that of freshwater. The term “brine” refers towater saturated or nearly saturated with salt and has a salinity that is50 ppt (parts per thousand) or greater. Brackish water is water that issaltier than fresh water, but not as salty as seawater, having asalinity ranging from 0.5 to 35 ppt. Seawater is water from a sea orocean and has a salinity ranging from 35 to 50 ppt. The saltwater sourcefrom which the carbonate mineral composition of the cements of theinvention is derived may be a naturally occurring source, such as a sea,ocean, lake, swamp, estuary, lagoon, deep brine, alkaline lakes, inlandseas, etc., or a man-made source.

Another type of water that may be employed in methods of the inventionis freshwater. Any suitable freshwater source may be used, includingsources ranging from relatively free of minerals to sources rich inminerals. Freshwater sources of interest include mineral rich freshwatersources. Mineral rich freshwater sources of interest may be naturallyoccurring, such as hard waters or lakes or inland seas, for examplealkaline lakes or inland seas (such as Lake Van in Turkey) which mayprovide a source of alkalinity for removal of protons and/or pH shiftand/or a source of minerals to be precipitated with the CO₂; such lakesare described further elsewhere herein. Mineral rich freshwater sourcesof interest may also be man-made, e.g., by producing a mineral richwater from a soft water. For example, a mineral poor (soft) water may becontacted with a source of desired ions, such as a calcium and/ormagnesium ion source, to produce a mineral rich water that is suitablefor use methods of the invention.

As indicated above, the alkaline-earth-metal-ion-containing wateremployed in methods of the invention may be a water that is obtainedfrom naturally occurring sources. Alternatively, the water may be onethat is prepared from an initial water, for example by adding one ormore minerals to the water. As such, some methods include preparing thealkaline-earth-metal containing water from an initial water by adding tothe initial water a source of one or more divalent metal ions, such asmagnesium, calcium, etc. Sources of magnesium ions include, but are notlimited, magnesium hydroxides, magnesium oxides, etc. Sources of calciumions include, but are not limited to, calcium hydroxides, calciumoxides, etc. Both naturally occurring and man-made sources of such ionsmay be employed. Specific naturally occurring sources of such ionsinclude, but are not limited to: mafic minerals, such as olivine,serpentine, periodotite, talc, etc., and the like. Addition ofsupplementary magnesium (Mg) ions to the source water, e.g., seawater,prior to precipitation increases yields of precipitate as well asaffects the composition of precipitate, providing a means for increasingCO₂ sequestration by utilizing minerals such as, but not limited to,Olivine, Serpentine and Mg(OH)₂ (Brucite). The particular Mg ion sourcemay be naturally occurring or man-made sources, and may be pure withrespect to the Mg mineral or impure, e.g., be a composition made up ofthe Mg mineral of interest and other minerals and components.

In some methods of the invention, the water (such as salt water ormineral rich water) is not contacted with a source of CO₂ prior tosubjecting the water to precipitation conditions. In these methods, thewater will have an amount of CO₂ associated with it, e.g., in the formof bicarbonate ion, which has been obtained from the environment towhich the water has been exposed prior to practice of the method.Subjecting the water to precipitation conditions of the inventionresults in conversion of this CO₂ into a storage stable precipitate, andtherefore sequestration of the CO₂. When the water subject to processesof the invention is again exposed to its natural environment, such asthe atmosphere, more CO₂ from the atmosphere will be taken up by thewater resulting in a net removal of CO₂ from the atmosphere andincorporation of a corresponding amount of CO₂ into a storage stableproduct, where the mineral rich freshwater source may be contacted witha source of CO₂, e.g., as described in greater detail below. Embodimentsof these methods may be viewed as methods of sequestering CO₂ gasdirectly from the Earth's atmosphere. Embodiments of the methods areefficient for the removal of CO₂ from the Earth's atmosphere. Forexample, embodiments of the methods are configured to remove CO₂ fromsaltwater at a rate of 0.025 M or more, such as 0.05 M or more,including 0.1 M or more per gallon of saltwater.

It will be appreciated by those of skill in the art that, althoughindustrial waste gas offers a relatively concentrated source of CO₂, themethods and systems of the invention are also applicable to removing CO₂from less concentrated sources, e.g., atmospheric air, which contains amuch lower concentration of CO₂ than, e.g., flue gas. Thus, in someembodiments the methods and systems of the invention encompassdecreasing the concentration of CO₂ in atmospheric air by producing astable precipitate, using the procedures outlined herein. In these casesthe concentration of CO₂ in the atmospheric air may be decreased by 10%or more, 20% or more, 30% or more, 40% or more, 50% or more, 60% ormore, 70% or more, 80% or more, 90% or more, 95% or more, 99% or more,99.9% or more, or 99.99%. Such decreases in atmospheric CO₂ may beaccomplished with yields as described herein, or with lower yields, andmay be accomplished in one precipitation step or in a series ofprecipitation steps.

In some embodiments, a source of CO₂ is contacted with analkaline-earth-metal containing water at some point during the method,such as before, during or even after the water has been subjected toprecipitation conditions of the invention. The source of CO₂ that iscontacted with the alkaline-earth-metal-ion containing water in theseembodiments may be any convenient CO₂ source. The CO₂ source may be aliquid, solid (e.g., dry ice), a supercritical fluid, or gaseous CO₂source.

In certain embodiments, the CO₂ source is a gaseous CO₂ source. Thisgaseous CO₂ source is, in certain instances, a waste feed from anindustrial plant. The nature of the industrial plant may vary in theseembodiments, where industrial plants of interest include power plants,chemical processing plants, mechanical processing plants, refineries,cement plants, steel plants, and other industrial plants that produceCO₂ as a byproduct of fuel combustion or other processing step (such ascalcination by a cement plant). By waste feed is meant a stream of gas(or analogous stream) that is produced as a byproduct of an activeprocess of the industrial plant. The gaseous stream may be substantiallypure CO₂ or a multi-component gaseous stream that includes CO₂ and oneor more additional gases. Multi-component gaseous streams (containingCO₂) that may be employed as a CO₂ source in embodiments of the subjectmethods include both reducing, e.g., syngas, shifted syngas, naturalgas, and hydrogen and the like, and oxidizing condition streams, e.g.,flue gases from combustion. Particular multi-component gaseous streamsof interest that may be treated according to the subject inventioninclude: oxygen containing combustion industrial plant flue gas, turbocharged boiler product gas, coal gasification product gas, shifted coalgasification product gas, anaerobic digester product gas, wellheadnatural gas stream, reformed natural gas or methane hydrates and thelike.

A variety of different gaseous waste streams may be treated according tomethods of the invention in order to sequester CO₂. Gaseous wastestreams of interest have, in certain embodiments, CO₂ present in amountsof 200 ppm to 1,000,000 ppm, such as 200,000 ppm to 1000 ppm andincluding 200,000 ppm to 2000 ppm, for example 130,000 ppm to 2000 ppm.The waste streams may include one or more additional components, e.g.,water, NOx (mononitrogen oxides; NO and NO₂), SOx (monosulfur oxides;SO, SO₂ and SO₃), VOC (Volatile organic compounds), mercury andparticulates (particulate matter, particles of solid or liquid suspendedin a gas).

The waste streams may be produced from a variety of different types ofindustrial plants. Of interest in certain embodiments are waste streamsproduced by industrial plants that combust fossil fuels, e.g., coal,oil, natural gas, as well as man-made fuel products of naturallyoccurring organic fuel deposits, such as but not limited to tar sands,heavy oil, oil shale, etc. In certain embodiments, power plants arepulverized coal power plants, supercritical coal power plants, mass burncoal power plants, fluidized bed coal power plants, gas or oil-firedboiler and steam turbine power plants, gas or oil-fired boiler simplecycle gas turbine power plants, and gas or oil-fired boiler combinedcycle gas turbine power plants. Of interest in certain embodiments arewaste streams produced by power plants that combust syngas, i.e., gasthat is produced by the gasification of organic matter, e.g., coal,biomass, etc., where in certain embodiments such plants are integratedgasification combined cycle (IGCC) plants. Of interest in certainembodiments are waste streams produced by Heat Recovery Steam Generator(HRSG) plants.

In some embodiments of the invention substantially 100% of the CO₂contained in a flue gas from a power plant is sequestered as a stablemineral; this may be done in a single precipitation step or in multipleprecipitation steps, and may further involve other processes forsequestering CO₂, e.g., as the concentration of CO₂ is decreased in theflue gas, more energy-intensive processes that be prohibitive in energyconsumption for removing all of the original CO₂ in the gas may becomepractical in removing the final CO₂ in the gas. Thus, in someembodiments, the gas entering the power plant (ordinary atmospheric air)may contain a concentration of CO₂ that is greater than theconcentration of CO₂ in the flue gas exiting the plant that has beentreated by the processes and systems of the invention. Hence, in someembodiments, the methods and systems of the invention encompass a methodcomprising supplying a gas, e.g., atmospheric air, to a power plant,where the gas comprises CO₂; treating the gas in the power plant, e.g.,by combustion of fossil fuel to consume O₂ and to produce CO₂ thentreating exhaust gas to remove CO₂; and releasing gas from the powerplant, where the gas released from the power plant has a lower CO₂content than the gas supplied to the power plant. In some embodiments,the gas released from the power plant contains at least 10% less CO₂, orat least 20% less CO₂, or at least 30% less CO₂, or at least 40% lessCO₂, or at least 50% less CO2, or at least 60% less CO₂, or at least 70%less CO₂, or at least 80% less CO₂, or at least 90% less CO₂, or atleast 95% less CO₂, or at least 99% less CO₂, or at least 99.5% lessCO₂, or at least 99.9% less CO₂, than the gas entering the power plant;in some embodiments the gas entering the power plant is atmospheric airand the gas exiting the power plant is treated flue gas.

Waste streams of interest also include waste streams produced by cementplants. Cement plants whose waste streams may be employed in methods ofthe invention include both wet process and dry process plants, whichplants may employ shaft kilns or rotary kilns, and may includepre-calciners. Each of these types of industrial plants may burn asingle fuel, or may burn two or more fuels sequentially orsimultaneously.

A waste stream of interest is industrial plant exhaust gas, e.g., a fluegas. By “flue gas” is meant a gas that is obtained from the products ofcombustion from burning a fossil or biomass fuel that are then directedto the smokestack, also known as the flue of an industrial plant. Inaddition to CO₂ generated by the burning of fuels, CO₂ can also bereleased as a result of other industrial processing (e.g., calcinationof minerals in a cement plant). The composition of the flue gas mayvary. In certain embodiments, the amount of CO₂ in the flue gas mayrange from 350 ppm to 400,000 ppm, such as 2000 ppm to 200,000 ppm andincluding 2000 ppm to 180,000 ppm. Other components may also be presentin the flue gas, e.g., water, NOx, SOx, VOC, mercury and particulates.The temperature of the flue gas may vary, e.g., from 0° C. to 2000° C.,such as from 60° C. to 7000° C. and including 100° C. to 400° C.

The gaseous waste stream employed in methods of the invention may beprovided from the industrial plant to the site of precipitation in anyconvenient manner that conveys the gaseous waste stream from theindustrial plant to the precipitation plant. In certain embodiments, thewaste stream is provided with a gas conveyer, e.g., a duct, which runsfrom a site of the industrial plant, e.g., a flue of the industrialplant, to one or more locations of the precipitation site. The source ofthe gaseous waste stream may be a distal location relative to the siteof precipitation, such that the source of the gaseous waste stream is alocation that is 1 mile or more, such as 10 miles or more, including 100miles or more, from the precipitation location. For example, the gaseouswaste stream may have been transported to the site of precipitation froma remote industrial plant via a CO₂ gas conveyance system, e.g., apipeline. The industrial plant generated CO₂ containing gas may or maynot be processed, e.g., remove other components, etc., before it reachesthe precipitation site (i.e., a carbonate compound precipitation plant).In yet other instances, source of the gaseous waste stream is proximalto the precipitation site, where such instances may include instanceswhere the precipitation site is integrated with the source of thegaseous waste stream, such as a power plant that integrates a carbonatecompound precipitation reactor.

Where desired, a portion of but less than the entire gaseous wastestream from the industrial plant may be employed in precipitationreaction. In these embodiments, the portion of the gaseous waste streamthat is employed in precipitation may be 75% or less, such as 60% orless and including 50% and less. In yet other embodiments, substantiallyall of the gaseous waste stream produced by the industrial plant, e.g.,substantially all of the flue gas produced by the industrial plant, isemployed in precipitation. In these embodiments, 80% or more, such as90% or more, including 95% or more, up to 100% of the gaseous wastestream (e.g., flue gas) generated by the source may be employed duringprecipitation.

As indicated above, the gaseous waste stream may be one that is obtainedfrom a flue or analogous structure of an industrial plant. In theseembodiments, a line, e.g., duct, is connected to the flue so that gasleaves the flue through the line and is conveyed to the appropriatelocation(s) of a precipitation system (described in greater detailbelow). Depending on the particular configuration of the portion of theprecipitation system at which the gaseous waste stream is employed, thelocation of the source from which the gaseous waste stream is obtainedmay vary, e.g., to provide a waste stream that has the appropriate ordesired temperature. As such, in certain embodiments where a gaseouswaste stream having a temperature ranging for 0° C. to 1800° C., such as60° C. to 700° C. is desired, the flue gas may be obtained at the exitpoint of the boiler or gas turbine, the kiln, or at any point throughthe power plant or stack, that provides the desired temperature. Wheredesired, the flue gas is maintained at a temperature above the dewpoint, e.g., 125° C., in order to avoid condensation and relatedcomplications. Where such is not possible, steps may be taken to reducethe adverse impact of condensation, e.g., employing ducting that isstainless steel, fluorocarbon (such as poly(tetrafluoroethylene)) lined,diluted with water and pH controlled, etc., so the duct does not rapidlydeteriorate.

To provide for efficiencies, the industrial plant that generates thegaseous waste stream may be co-located with the precipitation system. By“co-located” is meant that the distances between the industrial plantand precipitation system range from 10 to 500 yards, such as 25 to 400yards, including 30 to 350 yards. Where desired, the precipitation andindustrial plants may be configured relative to each other to minimizetemperature loss and avoid condensation, as well as minimize ductingcosts, e.g., where the precipitation plant is located within 40 yards ofthe industrial plant.

Also of interest in certain embodiments is a fully integrated plant thatincludes an industrial function (such as power generation, cementproduction, etc.) and a precipitation system of the invention. In suchintegrated plants, conventional industrial plants and precipitationsystem, such as described below, are modified to provide for the desiredintegrated plant. Modifications include, but are not limited to:coordination of stacks, pumping, controls, instrumentation, monitoring,use of plant energy, e.g., steam turbine energy to run portions of theprecipitation component, e.g., mechanical press, pumps, compressors, useof heat from cement and/or power plant obtained from steam or heat fromair to air heat exchanger, etc.

The pH of the water that is contacted with the CO₂ source may vary. Insome instances, the pH of the water that is contacted with the CO₂source is acidic, such that the pH is lower than 7, such as 6.5 orlower, 6 or lower, 5.5 or lower, 5 or lower, 4.5 or lower, 4 or lower.In yet other embodiments, the pH of the water may be neutral to slightlybasic, by which is meant that the pH of the water may range from 7 to 9,such as 7 to 8.5, including 7.5 to 8.5

In some instances, the water, such asalkaline-earth-metal-ion-containing water (including alkaline solutionsor natural saline alkaline waters), is basic when contacted with the CO₂source, such as a carbon dioxide containing gaseous stream. In theseinstances, while being basic the pH of the water is insufficient tocause precipitation of the storage stable carbon dioxide sequesteringproduct. As such, the pH may be 9.5 or lower, such as 9.3 or lower,including 9 or lower.

In some instances, the pH as described above may be maintained at asubstantially constant value during contact with the carbon dioxidecontaining gaseous stream, or the pH may be manipulated to maximize CO₂absorption while minimizing base consumption or other means of removingprotons, such as by starting at a certain pH and gradually causing thepH to rise as CO₂ continues to be introduced. In embodiments where thepH is maintained substantially constant, where by “substantiallyconstant” is meant that the magnitude of change in pH during some phaseof contact with the carbon dioxide source is 0.75 or less, such as 0.50or less, including 0.25 or less, such as 0.10 or less. The pH may bemaintained at substantially constant value, or manipulated to maximizeCO₂ absorption but prevent hydroxide precipitation withoutprecipitation, using any convenient approach. In some instances, the pHis maintained at substantially constant value, or manipulated tomaximize CO₂ absorption without precipitation, during CO₂ charging ofthe water by adding a sufficient amount of base to the water in a mannerthat provides the substantially constant pH. Any convenient base orcombination of bases may be added, including but not limited to oxidesand hydroxides, such as magnesium hydroxide, where further examples ofsuitable bases are reviewed below. In yet other instances, the pH may bemaintained at substantially constant value, or manipulated to maximizeCO₂ absorption, through use of electrochemical protocols, such as theprotocols described below, so that the pH of the water iselectrochemically maintained at the substantially constant value.Surprisingly, as shown in Example IV, it has been found that it ispossible to absorb, e.g., more than 50% of the CO₂ contained in a gascomprising about 20% CO₂ through simple sparging of seawater withaddition of base (removal of protons).

In some embodiments, the methods and systems of the invention arecapable of absorbing 5% or more, 10% or more, 15% or more, 20% or more,25% or more 30% or more, 35% or more, 40% or more, 45% or more, 50% ormore, 55% or more, 60% or more, 65% or more, 70% or more, 75% or more,80% or more, 85% or more, 90% or more, 95% or more, or 99% or more ofthe CO₂ in a gaseous source of CO₂, such as an industrial source of CO₂,e.g., flue gas from a power plant or waste gas from a cement plant. Insome embodiments, the methods and systems of the invention are capableof absorbing 50% or more of the CO₂ in a gaseous source of CO₂, such asan industrial source of CO₂, e.g., flue gas from a power plant or wastegas from a cement plant.

In addition to charging the initial water with CO₂, e.g., as describedabove, some embodiments of the methods include adding a magnesium ionsource to the initial water in a manner sufficient to produce amagnesium to calcium ratio in the water of 3 or higher, e.g., 4 orhigher, such as 5 or higher, for example 6 or higher, including 7 orhigher. In certain embodiments, the desired magnesium to calcium ionratio ranges from 3 to 10, such as 4 to 8. Any convenient magnesium ionsource may be added to the water to provide the desired magnesium tocalcium ion ratio, where specific magnesium ion sources of interestinclude, but are not limited to: Mg(OH)₂, serpentine, olivine, maficminerals, and ultramafic minerals. The amount of magnesium ion sourcethat is added to the water may vary, e.g., depending on the specificmagnesium ion source and the initial water from which the CO₂ chargedwater is produced. In certain embodiments, the amount of magnesium ionthat is added to the water ranges from 0.01 to 100.0 grams/liter, suchas from 1 to 100 grams/liter of water, including from 5 to 100grams/liter of water, for example from 5 to 80 grams/liter of water,including from 5 to 50 grams/liter of water. In certain embodiments, theamount of magnesium ion added to the water is sufficient to producewater with a hardness reading of about 0.06 grams/liter or more, such asabout 0.08 grams/liter or more, including about 0.1 grams/liter or moreas determined a Metrohm Titrator (Metrohm AG, Switzerland) according tomanufacturer's instructions. The magnesium ion source may be combinedwith the water using any convenient protocol, e.g. with agitation,mixing, etc.

In embodiments where a source of magnesium, calcium, or a combination ofmagnesium and calcium is added to the water, the source may be in solidform e.g., in the form of large, hard, and often crystalline particlesor agglomerations of particles that are difficult to get into solution.For example, Mg(OH)₂ as brucite can be in such a form, as are manyminerals useful in embodiments of the invention, such as serpentine,olivine, and other magnesium silicate minerals, as well as cement wasteand the like. Any suitable method may be used to introduce divalentcations such as magnesium from such sources into aqueous solution in aform suitable for reaction with carbonate to form carbonates of divalentcations. Increasing surface area by reducing particle size is one suchmethod, which can be done by means well known in the art such as ballgrinding and jet milling. Jet milling has the further advantage ofdestroying much of the crystal structure of the substance, enhancingsolubility. Also of interest is sonochemistry, where intense sonicationmay be employed to increase reaction rates by a desired amount, e.g.,10⁶× or more. The particles, with or without size reduction, may beexposed to conditions which promote aqueous solution, such as exposureto an acid such as HCl, H₂SO₄, or the like; a weak acid or a base mayalso be used in some embodiments. See, e.g., U.S. Patent PublicationNos. 2005/0022847; 2004/0213705; 2005/0018910; 2008/0031801; and2007/0217981; European Patent Nos. EP1379469; and EP1554031; and PCTPublication Nos. WO 07/016,271 and WO 08/061,305, all of which areincorporated by reference herein in their entirety.

In some embodiments the methods and systems of the invention utilizeserpentine as a mineral source. Serpentine is an abundant mineral thatoccurs naturally and may be generally described by the formula ofX₂₋₃Si₂O₅(OH)₄, wherein X is selected from the following: Mg, Ca, Fe²⁺,Fe³⁺, Ni, Al, Zn, and Mn, the serpentine material being a heterogeneousmixture consisting primarily of magnesium hydroxide and silica. In someembodiments of the invention, serpentine is used not only as a source ofmagnesium, but also as a source of hydroxide. Thus in some embodimentsof the invention, hydroxide is provided for removal of protons fromwater and/or adjustment of pH by dissolving serpentine; in theseembodiments an acid dissolution is not ideal to accelerate dissolution,and other means are used, such as jet milling and/or sonication. It willbe appreciated that in a batch or continuous process, the length of timeto dissolve the serpentine or other mineral is not critical, as once theprocess is started at the desired scale, and sufficient time has passedfor appropriate levels of dissolution, a continuous stream of dissolvedmaterial may be maintained indefinitely. Thus, even if dissolution tothe desired level takes days, weeks, months, or even years, once theprocess has reached the first time point at which desired dissolutionhas occurred, it may be maintained indefinitely. Prior to the timepointat which desired dissolution has occurred, other processes may be usedto provide some or all of the magnesium and/or hydroxide to the process.Serpentine is also a source of iron, which is a useful component ofprecipitates that are used for, e.g., cements, where iron components areoften desired.

Other examples of silicate-based minerals useful in the inventioninclude, but are not limited to olivine, a natural magnesium-ironsilicate ((Mg, Fe)₂SiO₄), which can also be generally described by theformula X₂(SiO₄)_(n), wherein X is selected from Mg, Ca, Fe²⁺, Fe³⁺, Ni,Al, Zn, and Mn, and n=2 or 3; and a calcium silicate, such aswollastonite. The minerals may be used individually or in combinationwith each other. Additionally, the materials may be found in nature ormay be manufactured. Examples of industrial by-products include but arenot limited to waste cement and calcium-rich fly ash.

In embodiments in which an electrochemical process is used to removeprotons and/or to produce base, often an acid stream, such as an HClstream, is also generated, and this stream, alone or any otherconvenient source of acid, or a combination thereof, may be used toenhance dissolution of, e.g., magnesium-bearing minerals such as olivineor serpentine, or sources of calcium such as cement waste. Dissolutionmay be further enhanced by sonication methods, which can producelocalized pockets of extreme temperature and pressure, enhancingreaction rates by one hundred to over one million-fold. Such methods areknown in the art.

In some embodiments the methods of the invention allow large amounts ofmagnesium and, in some cases, calcium, to be added to the water used insome embodiments of the invention, increasing the amount of precipitatethat may be formed per unit of water in a single precipitation step,allowing surprisingly high yields of carbonate-containing precipitatewhen combined with methods of dissolution of CO₂ from an industrialsource in water, e.g., seawater or other saltwater source. In someembodiments, the methods of the invention include a method of removingCO₂ from a gaseous source, e.g., an industrial gaseous source of CO₂such as flue gas from a power plant, or such as exhaust gas from acement plant, by performing a precipitation step on water into which CO₂has been dissolved from the gaseous source of CO₂, where theprecipitation step provides precipitate in an amount of 10 g/L or morein a single precipitation step, 15 g/L or more in a single precipitationstep, 20 g/L or more in a single precipitation step, 25 g/L or more in asingle precipitation step, 30 g/L or more in a single precipitationstep, 40 g/L or more in a single precipitation step, 50 g/L or more in asingle precipitation step, 60 g/L or more in a single precipitationstep, 70 g/L or more in a single precipitation step, 80 g/L or more in asingle precipitation step, 90 g/L or more in a single precipitationstep, 100 g/L or more in a single precipitation step, 125 g/L or more ina single precipitation step, or 150 g/L or more in a singleprecipitation step, In some embodiments the precipitate comprisesmagnesium carbonate; in some embodiments the precipitate comprisescalcium carbonate; in some embodiments, the precipitate comprisesmagnesium and calcium, and/or magnesium/calcium carbonates. In someembodiments the ratio of magnesium to calcium in the precipitatedmaterial produced in a single precipitation step is at least 0.5:1, orat least 1:1, or at least 2:1, or at least 3:1, or at least 4:1, or atleast 5:1, or at least 6:1, or at least 7:1, or at least 8:1, or atleast 9:1, or at least 10:1. In some embodiments the ratio of magnesiumto calcium in the precipitated material produced in a singleprecipitation step is at least 2:1. In some embodiments the ratio ofmagnesium to calcium in the precipitated material produced in a singleprecipitation step is at least 4:1. In some embodiments the ratio ofmagnesium to calcium in the precipitated material produced in a singleprecipitation step is at least 6:1. In some embodiments, the precipitatecontains calcium and magnesium carbonates, and contains components thatallow at least a portion of the carbon in the carbonate to be tracedback to a fossil fuel origin.

As reviewed above, methods of the invention include subjecting water(which may or may not have been charged with CO₂, as described above) toprecipitation conditions sufficient to produce a storage stableprecipitated carbon dioxide sequestering product. Any convenientprecipitation conditions may be employed, which conditions result in theproduction of the desired sequestering product.

Precipitation conditions of interest include those that modulate thephysical environment of the water to produce the desired precipitateproduct. For example, the temperature of the water may be raised to anamount suitable for precipitation of the desired product to occur. Insuch embodiments, the temperature of the water may be raised to a valuefrom 5 to 70° C., such as from 20 to 50° C. and including from 25 to 45°C. As such, while a given set of precipitation conditions may have atemperature ranging from 0 to 100° C., the temperature may be raised incertain embodiments to produce the desired precipitate. The temperatureof the water may be raised using any convenient protocol. In someinstances, the temperature is raised using energy generated from low orzero carbon dioxide emission sources, e.g., solar energy sources, windenergy sources, hydroelectric energy sources, geothermal energy sources,from the waste heat of the flue gas which can range up to 500° C., etc.

While the pH of the water may range from 7 to 14 during a givenprecipitation process, in some instances the pH is raised to alkalinelevels in order to produce the desired precipitation product. In theseembodiments, the pH is raised to a level sufficient to causeprecipitation of the desired CO₂ sequestering product, as describedabove. As such, the pH may be raised to 9.5 or higher, such as 10 orhigher, including 10.5 or higher. Where desired, the pH may be raised toa level which minimizes if not eliminates CO₂ production duringprecipitation. For example, the pH may be raised to a value of 10 orhigher, such as a value of 11 or higher. In certain embodiments, the pHis raised to between 7 and 11, such as between 8 and 11, includingbetween 9 and 11, for example between 10 and 11. In this step, the pHmay be raised to and maintained at the desired alkaline level, such thatthe pH is maintained at a constant alkaline level, or the pH may betransitioned or cycled between two or more different alkaline levels, asdesired.

The pH of the water may be raised using any convenient approach.Approaches of interest include, but are not limited to: use of a pHraising agent, electrochemical approaches, using naturally alkalinewater such as from an alkaline lake, etc. In some instances, a pHraising agent may be employed, where examples of such agents includeoxides (such as calcium oxide, magnesium oxide, etc.), hydroxides (suchas sodium hydroxide, potassium hydroxide, and magnesium hydroxide),carbonates (such as sodium carbonate) and the like. The amount of pHelevating agent which is added to the water will depend on theparticular nature of the agent and the volume of water being modified,and will be sufficient to raise the pH of the water to the desiredvalue.

In some embodiments, a source of an agent for removal of protons, duringdissolution of CO₂ and/or during the precipitation step in which pH israised, may be a naturally-occurring source. For example, in someembodiments the agent may comprise serpentine dissolved into aqueoussolution, as described above. In other embodiments the agent maycomprise a natural body of highly alkaline water. Such bodies of waterare well-known and are sources of large amounts of alkalinity, e.g.,Lake Van in Turkey has an average pH of 9.7-9.8. In addition, flyash,slag, cement waste, and other industrial wastes can provide sufficientalkalinity to remove at least a portion of the protons and/or provide asufficient pH change for precipitation.

In addition or as an alternative, protons may be removed from the water,e.g. while CO₂ is dissolved and/or at the precipitation step, usingelectrochemical approaches, which may remove protons without productionof hydroxide (e.g., if proton production from CO₂ dissolution matches orexceeds proton removal by an electrochemical process) or with productionof hydroxide. For example, electrodes (cathode and anode) may beprovided in the reactor which holds the water source, where theelectrodes may be separated by a selective barrier, such as a membrane,as desired. Where desired, byproducts of the hydrolysis product, e.g.,H₂, sodium metal, etc. may be harvested and employed for other purposes,as desired. Additional electrochemical approaches of interest include,but are not limited, those described in U.S. Provisional ApplicationSer. Nos. 61/081,299 and 61/091,729; the disclosures of which are hereinincorporated by reference.

In some instances, low-voltage electrochemical protocols are employedremove protons from the water, e.g. while CO₂ is dissolved and at theprecipitation step. By “low-voltage” is meant that the employedelectrochemical protocol operates at an average voltage of 2, 1.9, 1.8,1.7, or 1.6 V or less, such as 1.5, 1.4, 1.3, 1.2, 1.1 V or less, suchas 1V or less, including 0.9V or less, 0.8V or less, 0.7V or less, 0.6Vor less, 0.5V or less, 0.4V or less, 0.3V or less, 0.2V or less, or 0.1Vor less. Of interest are electrochemical protocols that do not generatechlorine gas. Also of interest are electrochemical protocols that do notgenerate oxygen gas. Also of interest are electrochemical protocols thatdo not generate hydrogen gas. In some instances, the electrochemicalprotocol is one that does not generate any gaseous by-byproduct.

Described below are two electrochemical processes and systems that maybe used in embodiments of the invention. The first makes use of ahydrogen transfer member that can act as both a cathode and an anode(i.e., a bielectrode). The second makes use of one or more ion-selectivemembranes (a low-voltage system for producing hydroxide). Theseprocesses and systems are further described in PCT Application No.PCT/US08/88242 entitled “Low-Energy Electrochemical Hydroxide System andMethod,” filed on Dec. 23, 2008, and PCT Application No. PCT/US08/88246entitled “Low-Energy Electrochemical Proton Transfer System and Method,”filed on Dec. 23, 2008; the disclosures of which are herein incorporatedby reference.

Bielectrode Methods and System

In various embodiments, the present method and system provides a lowenergy source of a deprotonated solution by positioning a hydrogentransfer member in an electrolytic cell wherein: on biasing a voltage ona first electrode positive relative to the hydrogen transfer member, anda second electrode in the cell negative relative to the hydrogentransfer member, a first electrolyte, in contact with the hydrogentransfer member and the first electrode, is deprotonated without formingoxygen or chlorine gas at the first electrode.

In one embodiment, the method comprises: positioning a conductivehydrogen transfer member to isolate a first electrolyte from a secondelectrolyte, the first electrolyte contacting a first electrode and thesecond electrolyte contacting a second electrode; and biasing a voltageon the first electrode positive relative to the hydrogen transfermember, and a voltage on the second electrode negative relative to thehydrogen transfer member to establish a current in the electrodes.

In an another embodiment, the method comprises: utilizing a hydrogentransfer member to isolate a first electrolyte from a secondelectrolyte; and biasing a voltage on a first electrode contacting thefirst electrolyte positive relative to the hydrogen transfer member; andbiasing a voltage on the second electrode contacting the secondelectrolyte negative relative to the hydrogen transfer member wherein,whereby protons are removed from the first electrolyte and introducedinto the second electrolyte.

In another embodiment, the system comprises: a first electrodecontacting a first electrolyte; a second electrode contacting in asecond electrolyte; a hydrogen transfer member isolating the firstelectrolyte from the second electrolyte; and a voltage regulatoroperable for biasing a voltage on the first electrode positive relativeto the hydrogen transfer member, and biasing a voltage on the secondelectrode negative relative to the hydrogen transfer member.

In another embodiment, the system comprises: a first electrolytic cellcomprising a first electrode contacting a first electrolyte; a secondelectrolytic cell comprising a second electrolyte contacting a secondelectrolyte; a hydrogen transfer member positioned to isolate the firstelectrolyte from the second electrolyte; a first conduit positioned forsupplying positive ions to the first electrolyte; a second conduitpositioned for supplying negative ions into the second electrolyte; anda voltage regulator operable to establish a current through theelectrodes by biasing a voltage on the first electrode positive relativeto the hydrogen transfer member, and a voltage on the second electrodenegative relative to the hydrogen transfer member.

In another embodiment, the method comprises forming a carbonate-ionenriched solution from a first electrolyte by contacting the firstelectrolyte with CO₂ while transferring hydrogen ions from the firstelectrolyte to a second electrolyte solution utilizing a hydrogentransfer member. In accordance with the method, a voltage regulator isoperable to establish a current through the electrodes by biasing avoltage on the first electrode positive relative to the hydrogentransfer member, and a voltage on the second electrode negative relativeto the hydrogen transfer member.

By the present system and method, protons are removed from the firstelectrolyte in contact with a first electrode, while protons areintroduced into another solution in contact with the second electrode(i.e., in some embodiments the pH of the first electrolyte in increasedand the pH of the other solution is decreased) without forming chlorineor oxygen gas on the first electrode. In one embodiment, the solutioncomprising removed protons has a decreased H⁺ concentration,corresponding to an increase OH⁻ concentration, and is useable insequestering CO₂ by precipitating calcium and magnesium carbonates andbicarbonates from a solution containing dissolved salts of these alkalimetals, as described further herein. Further, the solution comprisingthe increase in H⁺ concentration is useable in preparing the alkalisolutions herein, and/or other industrial applications.

The bielectrode described herein is directed to electrochemical systemsand methods for transferring H+ from one electrolyte solution toanother. Thus, by transferring H⁺ between aqueous electrolyticsolutions, the concentration of H⁺ in one solution may decrease, i.e.the solution becomes more basic, while the concentration of H⁺ in theother solution also increases i.e., the solution become more acidic.Alternatively, if one solution contains a proton source or a protonsink, the pH my not change, or may change more slowly, or even change inthe opposite direction from that predicted by proton removal oraddition.

In various embodiments, the methods and apparatus produce a basicsolution and an acidic solution. In various embodiments, the basicsolution is useable to sequester CO₂, and the acidic solution is useableto dissolve calcium and magnesium bearing minerals to provide calciumand magnesium ions for sequestering CO₂, as described further herein. Invarious embodiments, a hydrogen transfer material, such as palladium,separates the solutions and serve as a hydrogen transfer medium. Also,in various embodiments the hydrogen transfer material functions as acentral electrode between an anode and a cathode in a bi-electrodeconfiguration.

FIGS. 7A-7B illustrate various embodiments of the present system. Theseembodiments are illustrative only and in no way limit the methods orapparatuses. The system is adaptable for batch and continuous processesas described herein. Referring to FIG. 7A, system in one embodimentcomprises a first electrode 702 contacting a first electrolyte 704; asecond electrode 706 contacting a second electrolyte 708; a hydrogentransfer member 770 contacting and isolating first electrolyte 704 fromsecond electrolyte 708; and voltage regulators 724A and 724B operablefor biasing a voltage on first electrode 702 positive relative tohydrogen transfer member 770, and biasing a voltage on second electrode706 negative relative to the hydrogen transfer member. In variousembodiments, the voltage regulator is set to a voltage such that a gas,e.g., oxygen or chlorine gas does not form at the first electrode.

In the embodiment illustrated in FIG. 7A, first electrode 702 and firstelectrolyte 704 are contained in a first electrolytic chamber or cell772; and second electrode 706 and second electrolyte 708 are containedin a second electrolytic chamber or cell 714. First electrolyte cell 712and second electrolytic cell 714 are defined by positioning hydrogentransfer member 710 to isolate first electrolyte 704 from secondelectrolyte 708. In various embodiments, first and second electrolyticcells 712, 714 are comprised of a reservoir 716 such as a tank, avessel, a chamber, bag or a conduit. As is illustrated in FIGS. 7A-7B,hydrogen transfer member 710 member may constitute an entire barrier 718between electrolytes 704, 708, or a portion thereof. In embodimentswhere hydrogen transfer member 710 constitutes only a portion of barrier718, the remainder of the barrier comprises an insulating material.

In various embodiments, hydrogen transfer material 710 comprises a noblemetal, a transition metal, a platinum group metal, a metal of GroupsIVB, VB, VIB, or VIII of the periodic table of elements, alloys of thesemetals, oxides of these metals, or combinations of any of the foregoing.Other exemplary materials include palladium, platinum, iridium, rhodium,ruthenium, titanium, zirconium, chromium, iron, cobalt, nickel,palladium-silver alloys, palladium-copper alloys or amorphous alloyscomprising one or more of these metals. In various embodiments, thehydrogen transfer member also comprises a non-porous materials from thetitanium and vanadium groups, or comprise complex hydrides of group one,two, and three light elements of the Periodic Table such as Li, Mg, B,and Al. In other embodiments, a non-conductive or poorly conductivematerial can be made conductive as needed to function as a hydrogentransfer member, e.g. with a thin metal coating that can be applied bysputter deposition. In various embodiments, the hydrogen storagematerial 710 comprises a supported film or foil. In some embodiments,the hydrogen storage material 710 comprises palladium.

In operation, first electrode 702 is disposed at least partially infirst electrolyte solution 704 and in contact therewith, and secondelectrode 706 is likewise disposed at least partially in secondelectrolyte solution 708 and in contact therewith.

In various embodiments the electrolyte solution in first electrolyticcell 712 comprises a conductive aqueous solution such as fresh water ora salt water including seawater, brine, or brackish fresh water.Similarly, in second cell 714, the electrolyte comprises a conductiveaqueous such as fresh water or a salt water including seawater, brine,or brackish fresh water as described herein. In either cell, thesolution may be obtained form a natural source, or artificially created,or a combination of a natural source that has been modified foroperation in the process and/or apparatus of the invention as describedherein.

In an embodiment illustrated in FIGS. 7A-7B, first electrolytic solution704 is enriched with cations ions obtained, for example, by selectivelydi-ionizing salt water. Similarly, electrolytic solution 708 is enrichedwith anions ions obtained, for example, by selectively di-ionizing saltwater. As is illustrated in FIG. 7A by adding positive ions, e.g.,sodium ions to first electrolytic solution 704, and suitably biasingfirst 702 and second 706 electrodes as described herein, protons areremoved from the first solution; if protons are not replenished, or arereplenished more slowly than they are removed, then the system providesa deprotonated first electrolyte 704. Further, by surrounding firstelectrode 702 with a porous material 720 to prevent mixing of cationsfrom first electrode 702 with other ions in first electrolytic cellsolution 704, these electrode cations can be recovered at secondelectrode 706 in the second electrolytic cell by surrounding secondelectrode 706 with recovered cations and adjusting the voltages in thesystem to preferentially plate out cations on second electrode 706.Although tin is the electrode material illustrated in FIG. 7A, it willbe appreciated that any suitable material may be used. Similarly byintroducing chloride ions in second electrolyte 708 wherein the protonconcentration increases, an acid solution e.g., hydrochloric acid isobtained in second electrolytic cell 714. It will be appreciated thatany suitable cationic and anionic species may be used, and thatselection of species will depend on operating requirements of thesystem, the acid desired in second electrolyte 708, and the like. Insome embodiments, the cation is sodium and the anion is chloride, asillustrated in FIG. 7A.

In various embodiments first electrode 702 comprises an anode, andsecond electrode 706 comprises a cathode. In various embodiments, firstelectrode 702 comprises a sacrificial anode comprising a materialcomprising iron, tin, magnesium, calcium or combinations thereof and amineral. Other exemplary materials include a mineral, such as a maficmineral e.g., olivine or serpentine that provides cations. Where amineral is used as a part of first electrode 702 and functions as asource of cations, the mineral is positioned on a chemically inertconductive carrier such as stainless steel or platinum. Any suitablemineral may be used and selection of the mineral is based on the cationor cations desired for release, availability, cost and the like.

The system also comprises a voltage regulator and/or power supply 724A,724B configured to bias first electrode 702 positive relative tohydrogen transfer member 710, and configured to bias second electrode706 negative to hydrogen transfer member 710. In various embodiments,power supply comprises two separate power supplies 724A, 724B asillustrated in FIGS. 7-8, one configured to bias the first electrodepositively relative to the membrane, and another configured to bias thesecond electrode negative relative to the hydrogen transfer member 710.

In operation, power supply 724A, 724B drives an electrochemical reactionin which, without intending to be bound by any theory, it is believedthat hydrogen ions in first electrolyte solution 704 are reduced toatomic hydrogen and adsorb on a surface of hydrogen transfer member 710in contact with first electrolyte 702. At least a portion of theadsorbed hydrogen is absorbed in the body of hydrogen transfer member710 and desorbs on a surface of hydrogen transfer member 710 into secondelectrolyte 708 in contact with hydrogen transfer member 710 as hydrogenions. Regardless of mechanism, the result of the electrochemicalreaction is removal of proton from first electrolyte 704, andintroduction of a proton into second electrolyte 708. In embodimentswherein first electrode 702 comprises an oxidizable material e.g. iron,electrode 702 is oxidized to release iron ions (e.g., Fe⁺² and/or Fe⁺³)into first electrolyte solution 704 to balance the reduction of thehydrogen ions in first electrolyte 704.

In the present system, voltages on electrodes 702, 706 are biasedrelative to hydrogen transfer member 710 such that a gas does not formon first electrode 702. Hence, wherein first electrolyte 704 compriseswater, oxygen does not form on first electrode 702. Similarly, whereinthe first electrolyte comprises chloride ions, e.g., an electrolytecomprising salt water, chlorine gas does not form on the firstelectrode.

Without being bound to any theory as to a mechanism for proton transferfrom first electrolyte 704 to second electrolyte 708, it is believedthat hydrogen ions present in first electrolyte 704 are reduced toatomic hydrogen and adsorbs on the surface of hydrogen transfer member710 in contact the first electrolyte. In the system, power supply 724Bdrives another reaction at the opposing surface of membrane 710 incontact with second electrolyte 708 such that hydrogen absorbed in thebody of hydrogen transfer member 710 is oxidized back to hydrogen ionsand are released into second electrolyte solution 708 as hydrogen ions.To balance the reaction in which the atomic hydrogen is oxidized back tohydrogen ions, electrons are taken up at second electrode 706, forinstance, by reducing a cation in second electrolytic solution 708. Forexample, where second electrolytic solution 708 comprises seawater, thendepending upon the applied voltage some or all of sodium, calcium,magnesium, and other ions can be reduced at second electrode 706 to forma coating thereon.

In various embodiments as illustrated in FIGS. 7A-7B, the systemcomprises a source of CO₂ 726 coupled to a gas injection system 728disposed in first cell 712. The gas injection system mixes a gasincluding CO₂ supplied by the source of CO₂ into first electrolytesolution 704. Exemplary sources of CO₂ are described herein, and caninclude flue gas from burning fossil fuel burning at power plants, orwaste gas from an industrial process e.g., cement manufacture or steelmanufacture, for example. In various embodiments, gas injection system728 can comprise a sparger or injection nozzle; however, any suitablemechanism and apparatus for introducing CO₂ into an aqueous solution, asknown in the art, may be used.

Referring to FIGS. 7A and 7B, the system in an alternative embodimentfurther comprises a conduit 730A positioned to supply a solution ofpositive ions to first electrolyte 704, and conduit 730B positioned tosupply negative ions to second electrolyte 708. In various embodiments,conduits 730A, 730B are adaptable for batch or continuous flow. Asillustrated in FIGS. 7A and 7B, the system comprises a firstelectrolytic cell 712 comprising a first electrode 702 contacting afirst electrolyte 704; a second electrolytic cell 714 comprising asecond electrode 706 contacting a second electrolyte 708; a hydrogentransfer member 710 positioned to isolate the first electrolyte from thesecond electrolyte; a first conduit 730A positioned for supplyingpositive ions to the first electrolyte; a second conduit 730B positionedfor supplying negative ions into the second electrolyte; and voltageregulators 724A, 724B operable to establish a current through electrodes702, 706 by biasing a voltage on first electrode 702 positive relativeto the hydrogen transfer member 710, and a voltage on the secondelectrode 706 negative relative to the hydrogen transfer member.

As will be appreciated by one skilled in the art, protons are removedfrom electrolyte solution 704 and introduced in to electrolyte solution708. In some embodiments, electrolyte solution 704 further includes asource of protons as illustrated in FIGS. 7A and 7B. In someembodiments, CO₂ gas may be introduced into electrolyte solution 704 andthrough well known chemistry, react with water to form a carbonic acidthat can dissociate to form a bicarbonate ion and a proton; and thebicarbonate ion may further dissociate to form a carbonate ion andanother proton.

Thus, in some embodiments, e.g., where CO₂ is introduced, protons areboth removed and introduced into electrolyte solution 704, and the netresult—net removal, no change, or net introduction of protons—willdepend on the relative rates of protons removal by the electrochemicalprocess and introduction by e.g., CO₂ introduction. Similarly, inelectrolyte solution 708, if there is a process that removes protonse.g., dissolution of a basic substance, then the net result inelectrolyte solution 708 may be introduction of, no change in, orremoval of protons.

In some embodiments, there is a net removal of protons (coupled withintroduction of cations) in electrolyte solution 704, and/or a netintroduction of protons (couple with introduction of anions, e.g.,chloride) in electrolyte solution 708. Thus, in some embodiments, acationic hydroxide, e.g. sodium hydroxide will be formed in firstelectrolyte solution 704 and/or hydrogen anion solution, e.g.,hydrochloric acid will be formed in second solution 708. Either or bothof cationic hydroxide e.g., sodium hydroxide, or the hydrogen anionicsolution e.g. hydrochloric acid can be withdrawn and used elsewhere,e.g., in the sequestration of carbon dioxide as describe above, and inother industrial applications.

The voltage across the electrodes used to remove protons from solutionmay be low. In various embodiments, the voltage across the electrodesmay be less than about 0.1, 0.2, 0.3, 0.4, 0.5, 0.6, 0.7, 0.8, 0.9, 1.0,1.1, 1.2, 1.3, 1.4, 1.5, 1.6, 1.7, 1.8, 1.9, 2.0, 2.1, or 2.2 V. In someembodiments, the voltage across the electrodes is less than about 2.0V.In some embodiments, the voltage across the electrodes is less thanabout 1.5V. In some embodiments, the voltage across the electrodes isless than about 1.0V. In some embodiments, the voltage across theelectrodes is less than about 0.8V. In some embodiments, the voltageacross the electrodes is less than about 0.6V. In some embodiments, thevoltage across the electrodes is less than about 0.4V.

Exemplary results achieved in accordance with the present system aresummarized in Table 1 below.

TABLE 1 Low Energy Electrochemical Method and System (Bi-electrode) Voltacross Time Initial pH End pH at Initial pH at End pH at Electrodes(min) Anode Anode Cathode Cathode 0.45 V 30 4.994 5.204 7.801 10. 7.431[0.15 V across the deprotonated solution; and 0.30 V across theprotonated solution]Low Voltage System for Production of Hydroxide

A second set of methods and systems for removing protons from aqueoussolution/producing hydroxide pertains to a low energy process forelectrochemically preparing an ionic solution utilizing an ion exchangemembrane in an electrochemical cell. In one embodiment, the systemcomprises an electrochemical system wherein an ion exchange membraneseparates a first electrolyte from a second electrolyte, the firstelectrolyte contacting an anode and the second electrolyte contacting acathode. In the system, on applying a voltage across the anode andcathode, hydroxide ions form at the cathode and a gas does not form atthe anode.

In an another embodiment, the system comprises an electrochemical systemcomprising a first electrolytic cell including an anode contacting afirst electrolyte, and an anion exchange membrane separating the firstelectrolyte from a third electrolyte; and a second electrolytic cellincluding a second electrolyte contacting a cathode and a cationexchange membrane separating the first electrolyte from the thirdelectrolyte; wherein on applying a voltage across the anode and cathode,hydroxide ions form at the cathode and a gas does not form at the anode.

In one embodiment the method comprises placing an ion exchange membranebetween a first electrolyte and a second electrolyte, the firstelectrolyte contacting an anode and the second electrolyte contacting acathode; and migrating ions across the ion exchange membrane by applyinga voltage across the anode and cathode to form hydroxide ions at thecathode without forming a gas at the anode.

In another embodiment the method comprises placing a third electrolytebetween an anion exchange membrane and a cation exchange membrane; afirst electrolyte between the anion exchange and an anode; and secondelectrolyte between the cation exchange membrane and a cathode; andmigrating ions across the cation exchange membrane and the anionexchange membrane by applying a voltage to the anode and cathode to formhydroxide ions at the cathode without forming a gas at the anode.

By the present methods and systems, ionic species from one solution aretransferred to another solution in a low voltage electrochemical manner,thereby providing anionic solutions for various applications, includingpreparing a solution of sodium hydroxide for use in sequestration carbondioxide as described herein. In one embodiment, a solution comprising ofis obtained from salt water and used in sequestering CO₂ byprecipitating calcium and magnesium carbonates and bicarbonates from asalt solution comprising alkaline earth metal ions as described herein.

The methods and systems in various embodiments are directed to a lowvoltage electrochemical system and method for generating a solution ofsodium hydroxide in an aqueous solution utilizing one or more ionexchange membranes wherein, a gas is not formed at the anode and whereinhydroxyl ions are formed at the cathode. Thus, in some embodiments,hydroxide ions are formed in an electrochemical process without theformation of oxygen or chlorine gas. In some embodiments, hydroxide ionsare formed in an electrochemical process where the voltage appliedacross the anode and cathode is less than 2.8, 2.7, 2.5, 2.4, 2.3, 2.2,2.1, 2.0, 1.9, 1.8, 1.7, 1.6, 1.5, 1.4, 1.3, 1.2, 1.1, 1.0, 0.9, 0.8,0.7, 0.6, 0.5, 0.4, 0.3, 0.2, or 0.1 V. In various embodiments, an ionicmembrane is utilized to separate a salt water in contact with the anode,from a solution of e.g., sodium chloride in contact with the cathode. Onapplying a low voltage across the cathode and anode, a solution of e.g.,sodium hydroxide is formed in the solution around the cathode;concurrently, an acidified solution comprising hydrochloric acid isformed in the solution around the anode. In various embodiments, a gassuch as chorine or oxygen does not form at the anode.

In various embodiments, the sodium hydroxide solution is useable tosequester CO₂ as described herein, and the acidic solution is useable todissolve calcium and magnesium bearing minerals to provide a calcium andmagnesium ions for sequestering CO₂, also as described herein.

Turning to FIGS. 8-10, in various embodiments the system is adaptablefor batch and continuous processes as described herein. Referring toFIGS. 8-9, in one embodiment the system includes an electrochemical cellwherein an ion exchange membrane (802, 824) is positioned to separate afirst electrolyte (804) from a second electrolyte (806), the firstelectrolyte contacting an anode (808) and the second electrolytecontacting a cathode (810). As illustrated in FIG. 8, an anion exchangemembrane (802) is utilized; in FIG. 9, a cation exchange membrane (824)is utilized.

In various embodiments as illustrated in FIGS. 8 and 9, firstelectrolyte (804) comprises an aqueous salt solution comprisingseawater, freshwater, brine, or brackish water or the like; and secondelectrolyte comprises a solution substantially of sodium chloride. Invarious embodiments, second (806) electrolyte may comprise seawater or aconcentrated solution of sodium chloride. In various embodiments anionexchange membrane (802) and cation exchange membrane (824) comprise aconventional ion exchange membranes suitable for use in an acidic and/orbasic solution at operating temperatures in an aqueous solution up toabout 100° C. As illustrated in FIGS. 8 and 9, first and secondelectrolytes are in contact with the anode and cathode to complete anelectrical circuit that includes voltage or current regulator (812). Thecurrent/voltage regulator is adaptable to increase or decrease thecurrent or voltage across the cathode and anode in the system asdesired.

With reference to FIGS. 8 and 9, in various embodiments, theelectrochemical cell includes first electrolyte inlet port (814)adaptable for inputting first electrolyte (804) into the system and incontact with anode (808). Similarly, the cell includes secondelectrolyte inlet port (816) for inputting second electrolyte (806) intothe system and in contact with cathode (810). Additionally, the cellincludes outlet port (818) for draining first electrolyte from the cell,and outlet port (820) for draining second electrolyte from the cell. Aswill be appreciated by one ordinarily skilled, the inlet and outletports are adaptable for various flow protocols including batch flow,semi-batch flow, or continuous flow. In alternative embodiments, thesystem includes a duct (822) for directing gas to the anode; in variousembodiments the gas comprises hydrogen formed at the cathode (810).

With reference to FIG. 8 where an anion membrane (802) is utilized, uponapplying a low voltage across the cathode (810) and anode (808),hydroxide ions form at the cathode (810) and a gas does not form at theanode (808). Further, where second electrolyte (806) comprises sodiumchloride, chloride ions migrate into the first electrolyte (804) fromthe second electrolyte (806) through the anion exchange membrane (802);protons form at the anode (808); and hydrogen gas forms at the cathode(810). As noted above, a gas e.g., oxygen or chlorine does not form atthe anode (808).

With reference to FIG. 9 where a cation membrane (824) is utilized, uponapplying a low voltage across the cathode (810) and anode (808),hydroxide ions form at the cathode (810) and a gas does not form at theanode (808). In various embodiments cation exchange membrane (824)comprises a conventional cation exchange membrane suitable for use withan acidic and basic solution at operating temperatures in an aqueoussolution up to about 100° C. As illustrated in FIG. 9, first and secondelectrolytes are in contact with the anode and cathode to complete anelectrical circuit that includes voltage and/or current regulator (812).The voltage/current regulator is adaptable to increase or decrease thecurrent or voltage across the cathode and anode in the system asdesired. In the system as illustrated in FIG. 9 wherein secondelectrolyte (806) comprises sodium chloride, sodium ions migrate intothe second electrolyte (806) from the first electrolyte (804) throughthe cation exchange membrane (824); protons form at the anode (808); andhydrogen gas forms at the cathode (810). As noted above, a gas e.g.,oxygen or chlorine does not form at the anode (808).

As can be appreciated by one ordinarily skilled in the art, and withreference to FIG. 8 in second electrolyte (806) as hydroxide ions fromthe anode (810) and enter in to the second electrolyte (806) concurrentwith migration of chloride ions from the second electrolyte, an aqueoussolution of sodium hydroxide will form in second electrolyte (806).Consequently, depending on the voltage applied across the system and theflow rate of the second electrolyte (806) through the system, the pH ofthe second electrolyte is adjusted. In one embodiment, when a potentialof about 0.1 V or less, 0.2 V or less, 0.3 V or less, 0.4 V or less, 0.5V or less, 0.6 V or less, 0.7 V or less, 0.8 V or less, 0.9 V or less,1.0 V or less, 1.1 V or less, 1.2 V or less, 1.3 V or less, 01.4 V orless, 1.5 V or less, 1.6 V or less, 1.7 V or less, 1.8 V or less, 1.9 Vor less, or 2.0 V or less, is applied across the anode and cathode, thepH of the second electrolyte solution increased; in another embodiment,when a volt of about 0.1 to 2.0 V is applied across the anode andcathode the pH of the second electrolyte increased; in yet anotherembodiment, when a voltage of about 0.1 to 1 V is applied across theanode and cathode the pH of the second electrolyte solution increased.Similar results are achievable with voltages of 0.1 to 0.8 V; 0.1 to 0.7V; 0.1 to 0.6 V; 0.1 to 0.5 V; 0.1 to 0.4 V; and 0.1 to 0.3 V across theelectrodes. Exemplary results achieved in accordance with the presentsystem are summarized in Table 2.

TABLE 2 Low Energy Electrochemical Method and System Volt across TimeInitial pH at End pH at Initial pH at End pH at Electrodes (sec) AnodeAnode Cathode Cathode 0.6 2000 6.7 3.8 6.8 10.8 1.0 2000 6.6 3.5 6.811.1

In this example, both the anode and the cathode comprise platinum, andthe first and second electrolytes comprise a solution of sodiumchloride.

Similarly, with reference to FIG. 9, in second electrolyte (806) ashydroxide ions from the anode (810) enter into the solution concurrentwith migration of sodium ions from the first electrolyte to the secondelectrolyte, increasingly an aqueous solution of sodium hydroxide willform in second electrolyte (806). Depending on the voltage appliedacross the system and the flow rate of the second electrolyte throughthe system, the pH of the solution will be adjusted. In one embodiment,when a voltage of about 0.1 V or less, 0.2 V or less, 0.3 V or less, 0.4V or less, 0.5 V or less, 0.6 V or less, 0.7 V or less, 0.8 V or less,0.9 V or less, 1.0 V or less, 1.1 V or less, 1.2 V or less, 1.3 V orless, 01.4 V or less, 1.5 V or less, 1.6 V or less, 1.7 V or less, 1.8 Vor less, 1.9 V or less, or 2.0 V or less is applied across the anode andcathode, the pH of the second electrolyte solution increased; in anotherembodiment, when a voltage of about 0.1 to 2.0 V is applied across theanode and cathode the pH of the second electrolyte increased; in yetanother embodiment, when a voltage of about 0.1.0 to 1 V is appliedacross the anode and cathode the pH of the second electrolyte solutionincreased. Similar results are achievable with voltages of 0.1 to 0.8 V;0.1 to 0.7 V; 0.1 to 0.6 V; 0.1 to 0.5 V; 0.1 to 0.4 V; and 0.1 to 0.3 Vacross the electrodes. In one embodiment, a voltage of about 0.6 V orless is applied across the anode and cathode; in another embodiment, avoltage of about 0.1 to 0.6 V or less is applied across the anode andcathode; in yet another embodiment, a voltage of about 0.1 to 1 V orless is applied across the anode and cathode.

In various embodiments and with reference to FIGS. 8-10, hydrogen gasformed at the cathode (810) is directed to the anode (808) where,without being bound to any theory, it is believed that the gas isadsorbed and/or absorbed into the anode and subsequently forms protonsat the anode. Accordingly, as can be appreciated, with the formation ofprotons at the anode and migration of e.g., chloride ions into the firstelectrolyte (804) as in FIG. 8, or migration of e.g., sodium ions fromthe first electrolyte as in FIG. 10, an acidic solution comprising e.g.,hydrochloric acid is obtained in the first electrolyte (804).

In another embodiment as illustrated in FIG. 10, the system inaccordance with the present invention comprises an electrochemical cellincluding anode (808) contacting first electrolyte (804) and an anionexchange membrane (802) separating the first electrolyte from a thirdelectrolyte (830); and a second electrolytic cell comprising a secondelectrolyte (806) contacting a cathode (880) and a cation exchangemembrane (824) separating the first electrolyte from the thirdelectrolyte, wherein on applying a voltage across the anode and cathode,hydrogen ions form at the cathode without a gas forming at the anode. Aswith the system of FIGS. 8 and 9, the system of FIG. 10 is adaptable forbatch and continuous processes.

In various embodiments as illustrated in FIG. 10, first electrolyte(804) and second electrolyte (806) comprise an aqueous salt solutioncomprising seawater, freshwater, brine, or brackish water or the like;and second electrolyte comprises a solution substantially of sodiumchloride. In various embodiments, first (804) and second (806)electrolytes may comprise seawater. In the embodiment illustrated inFIG. 10, the third electrolyte (830) comprises substantially sodiumchloride solution.

In various embodiments anion exchange membrane (802) comprises anysuitable anion exchange membrane suitable for use with an acidic andbasic solution at operating temperatures in an aqueous solution up toabout 100° C. Similarly, cation exchange membrane (824) comprises anysuitable cation exchange membrane suitable for use with an acidic andbasic solution at operating temperatures in an aqueous solution up toabout 100° C.

As illustrated in FIG. 10, in various embodiments first electrolyte(804) is in contact with the anode (808) and second electrolyte (806) isin contact with the cathode (810). The third electrolyte (830), incontact with the anion and cation exchange membrane, completes anelectrical circuit that includes voltage or current regulator (812). Thecurrent/voltage regulator is adaptable to increase or decrease thecurrent or voltage across the cathode and anode in the system asdesired.

With reference to FIG. 10, in various embodiments, the electrochemicalcell includes first electrolyte inlet port (814) adaptable for inputtingfirst electrolyte 804 into the system; second electrolyte inlet port(816) for inputting second electrolyte (806) into the system; and thirdinlet port (826) for inputting third electrolyte into the system.Additionally, the cell includes outlet port (818) for draining firstelectrolyte; outlet port (820) for draining second electrolyte; andoutlet port (828) for draining third electrolyte. As will be appreciatedby one ordinarily skilled, the inlet and outlet ports are adaptable forvarious flow protocols including batch flow, semi-batch flow, orcontinuous flow. In alternative embodiments, the system includes a duct(822) for directing gas to the anode; in various embodiments the gas ishydrogen formed at the cathode (810).

With reference to FIG. 10, upon applying a low voltage across thecathode (810) and anode (808), hydroxide ions form at the cathode (810)and a gas does not form at the anode (808). Further, where thirdelectrolyte (830) comprises sodium chloride, chloride ions migrate intothe first electrolyte (804) from the third electrolyte (830) through theanion exchange membrane (802); sodium ions migrate to the secondelectrolyte (806) from the third electrolyte (830); protons form at theanode; and hydrogen gas forms at the cathode. As noted previously, a gase.g., oxygen or chlorine does not form at the anode (808).

As can be appreciated by one ordinarily skilled in the art, and withreference to FIG. 10 in second electrolyte (806) as hydroxide ions fromthe cathode (810) enter into the solution concurrent with migration ofsodium ions from the third electrolyte, increasingly an aqueous solutionof sodium hydroxide will form in second electrolyte (806). Depending onthe voltage applied across the system and the flow rate of the secondelectrolyte through the system, the pH of the solution will be adjusted.In one embodiment, when a voltage of about 0.1 V or less, 0.2 V or less,0.3 V or less, 0.4 V or less, 0.5 V or less, 0.6 V or less, 0.7 V orless, 0.8 V or less, 0.9 V or less, 1.0 V or less, 1.1 V or less, 1.2 Vor less, 1.3 V or less, 01.4 V or less, 1.5 V or less, 1.6 V or less,1.7 V or less, 1.8 V or less, 1.9 V or less, or 2.0 V or less or less isapplied across the anode and cathode, the pH of the second electrolytesolution increased; in another embodiment, when a voltage of about 0.1to 2.0 V is applied across the anode and cathode the pH of the secondelectrolyte increased; in yet another embodiment, when a voltage ofabout 0.1.0 to 1 V is applied across the anode and cathode the pH of thesecond electrolyte solution increased. Similar results are achievablewith voltages of 0.1 to 0.8 V; 0.1 to 0.7 V; 0.1 to 0.6 V; 0.1 to 0.5 V;0.1 to 0.4 V; and 0.1 to 0.3 V across the electrodes. In one embodiment,a voltage of about 0.6 V or less is applied across the anode andcathode; in another embodiment, a voltage of about 0.1 to 0.6 V or lessis applied across the anode and cathode; in yet another embodiment, avoltage of about 0.1 to 1 V or less is applied across the anode andcathode.

Similarly, with reference to FIG. 10, in first electrolyte (804) asprotons form at the anode (808) and enter into the solution concurrentwith migration of chloride ions from the third electrolyte to the firstelectrolyte, increasingly an acidic solution will form in firstelectrolyte (804). Depending on the voltage applied across the systemand the flow rate of the second electrolyte through the system, the pHof the solution will be adjusted. In one embodiment, when a voltage ofabout 0.1 V or less, 0.2 V or less, 0.3 V or less, 0.4 V or less, 0.5 Vor less, 0.6 V or less, 0.7 V or less, 0.8 V or less, 0.9 V or less, 1.0V or less, 1.1 V or less, 1.2 V or less, 1.3 V or less, 01.4 V or less,1.5 V or less, 1.6 V or less, 1.7 V or less, 1.8 V or less, 1.9 V orless, or 2.0 V or less is applied across the anode and cathode, the pHof the second electrolyte solution increased; in another embodiment,when a voltage of about 0.1 to 2.0 V is applied across the anode andcathode the pH of the second electrolyte increased; in yet anotherembodiment, when a voltage of about 0.1.0 to 1 V is applied across theanode and cathode the pH of the second electrolyte solution increased.Similar results are achievable with voltages of 0.1 to 0.8 V; 0.1 to 0.7V; 0.1 to 0.6 V; 0.1 to 0.5 V; 0.1 to 0.4 V; and 0.1 to 0.3 V across theelectrodes. In one embodiment, a voltage of about 0.6 V or less isapplied across the anode and cathode; in another embodiment, a voltageof about 0.1 to 0.6 V or less is applied across the anode and cathode;in yet another embodiment, a voltage of about 0.1 to 1 V or less isapplied across the anode and cathode as indicated in Table 2.

As illustrated in FIG. 10, hydrogen gas formed at the cathode (810) isdirected to the anode (808) where, without being bound to any theory, itis believed that hydrogen gas is adsorbed and/or absorbed into the anodeand subsequently forms protons at the anode and enters the firstelectrolyte (804). Also, in various embodiments as illustrated in FIGS.8-10, a gas such as oxygen or chlorine does not form at the anode (808).Accordingly, as can be appreciated, with the formation of protons at theanode and migration of chlorine into the first electrolyte, hydrochloricacid is obtained in the first electrolyte (804).

As described with reference to FIGS. 8-9, as hydroxide ions from theanode (810) and enter in to the second electrolyte (806) concurrent withmigration of chloride ions from the second electrolyte, an aqueoussolution of sodium hydroxide will form in second electrolyte (806).Consequently, depending on the voltage applied across the system and theflow rate of the second electrolyte (806) through the system, the pH ofthe second electrolyte is adjusted. In one embodiment, when a voltage ofabout 0.1 V or less, 0.2 V or less, 0.3 V or less, 0.4 V or less, 0.5 Vor less, 0.6 V or less, 0.7 V or less, 0.8 V or less, 0.9 V or less, 1.0V or less, 1.1 V or less, 1.2 V or less, 1.3 V or less, 01.4 V or less,1.5 V or less, 1.6 V or less, 1.7 V or less, 1.8 V or less, 1.9 V orless, or 2.0 V or less is applied across the anode and cathode, the pHof the second electrolyte solution increased; in another embodiment,when a voltage of about 0.1 to 2.0 V is applied across the anode andcathode the pH of the second electrolyte increased; in yet anotherembodiment, when a voltage of about 0.1.0 to 1 V is applied across theanode and cathode the pH of the second electrolyte solution increased.Similar results are achievable with voltages of 0.1 to 0.8 V; 0.1 to 0.7V; 0.1 to 0.6 V; 0.1 to 0.5 V; 0.1 to 0.4 V; and 0.1 to 0.3 V across theelectrodes. In one embodiment, when a voltage of about 0.6 V or less isapplied across the anode and cathode, the pH of the second electrolytesolution increased; in another embodiment, when a voltage of about 0.1to 0.6 V or less is applied across the anode and cathode the pH of thesecond electrolyte increased; in yet another embodiment, when a voltageof about 0.1 to 1 V or less is applied across the anode and cathode thepH of the second electrolyte solution increased.

Optionally, a gas including CO₂ is dissolved into the second electrolytesolution by bubbling the gas into the first electrolyte solution 804 asdescribe above. In an optional step the resulting second electrolytesolution is used to precipitate a carbonate and/or bicarbonate compoundsuch as calcium carbonate or magnesium carbonate and or theirbicarbonates, as described herein. The precipitated carbonate compoundcan be used as cements and build material as described herein.

In another optional step, acidified second electrolyte solution 804 isutilized to dissolve a calcium and/or magnesium rich mineral, such asmafic mineral including serpentine or olivine for use as the solutionfor precipitating carbonates and bicarbonates as described herein. Invarious embodiments, the resulting solution can be used as the secondelectrolyte solution. Similarly, in embodiments where hydrochloric acidis produced in second electrolyte 806, the hydrochloric acid can be usedin place of, or in addition to, the acidified second electrolytesolution.

Embodiments described above produce electrolyte solutions enriched inbicarbonate ions and carbonate ions, or combinations thereof as well asan acidified stream. The acidified stream can also find application invarious chemical processes. For example, the acidified stream can beemployed to dissolve calcium and/or magnesium rich minerals such asserpentine and olivine to create the electrolyte solution used in thereservoir 816. Such an electrolyte solution can be charged withbicarbonate ions and then made sufficiently basic so as to precipitatecarbonate compounds as described herein.

In some embodiments, a first electrochemical process may be used toremove protons from solution to facilitate CO₂ absorption, withoutconcomitant production of hydroxide, while a second electrochemicalprocess may be used to produce hydroxide in order to further removeprotons to shift equilibrium toward carbonate and cause precipitation ofcarbonates. The two processes may have different voltage requirements,e.g., the first process may require lower voltage than the second, thusminimizing total overall voltage used in the process. For example, thefirst process may be a bielectrode process as described above, operatingat 1.0V or less, or 0.9V or less, or 0.8V or less, or 0.7V or less, or0.6V or less, or 0.5V or less, or 0.4V or less, or 0.3V or less, or 0.2Vor less, or 0.1V or less, while the second process may be a low-voltagehydroxide producing process as described above, operating at 1.5 V orless, or 1.4V or less, or 1.3V or less, or 1.2V or less, or 1.1 V orless, 1.0V or less, or 0.9V or less, or 0.8V or less, or 0.7V or less,or 0.6V or less, or 0.5V or less, or 0.4V or less, or 0.3V or less, or0.2V or less, or 0.1V or less. For example, in some embodiments thefirst process is a bielectrode process operating at 0.6 V or less andthe second process is a low-voltage hydroxide producing processoperating at 1.2V or less.

Also of interest are the electrochemical approaches described inpublished United States Application Publication Nos. 20060185985 and20080248350, as well as published PCT Application Publication No. WO2008/018928; the disclosures of which are hereby incorporated byreference.

Stoichiometry dictates that the production of a carbonate to beprecipitated in order to sequester CO₂ from a source of CO₂ requires theremoval of two protons from the initial carbonic acid that is formedwhen CO₂ is dissolved in water (see equations 1-5, above). Removal ofthe first proton produces bicarbonate and removal of the second producescarbonate, which may be precipitated as, e.g., a carbonate of a divalentcation, such as magnesium carbonate or calcium carbonate. The removal ofthe two protons requires some process or combination of processes whichtypically require energy. For example, if the protons are removedthrough the addition of sodium hydroxide, the source of renewable sodiumhydroxide is typically the chloralkali process, which uses anelectrochemical process requiring at least 2.8 V and a fixed amount ofelectrons per mole of sodium hydroxide. That energy requirement may beexpressed in terms of a carbon footprint, i.e., amount of carbonproduced to provide the energy to drive the process.

A convenient way of expressing the carbon footprint for a given processof proton removal is as a percentage of the CO₂ removed from the sourceof CO₂. That is, the energy required for the removal of the protons maybe expressed in terms of CO₂ emission of a conventional method of powergeneration to produce that energy, which may in turn be expressed as apercent of the CO₂ removed from the source of CO₂. For convenience, andas a definition in this aspect of the invention, the “CO₂ produced” insuch a process will be considered the CO₂ that would be produced in aconventional coal/steam power plant to provide sufficient energy toremove two protons. Data are publicly available for such power plantsfor the last several years that show tons of CO₂ produced per total MWhof energy produced. For purposes of definition here, a value of 1 tonCO₂ per MWh will be used, which corresponds closely to typicalcoal-fired power plants; for example, the WA Parish plant produced18,200,000 MWh of energy in 2000 while producing approximately19,500,000 tons of CO₂ and at present produces 21,300,00 MWh of energywhile producing 20,900,000 tons of CO₂, which average out very close tothe definitional 1 ton CO₂ per MWh that will be used herein. Thesenumbers can then be used to calculate the CO₂ production necessary toremove sufficient protons to remove CO₂ from a gas stream, and compareit to the CO₂ removed. For example, in a process utilizing thechloralkali process operating at 2.8 V to provide base, and used tosequester CO2 from a coal/stem power plant, the amount of CO₂ producedby the power plant to supply the energy to create base by thechloralkali process to remove two protons, using the 1 ton CO₂/1 MWhratio, would be well above 200% of the amount of CO₂ sequestered by theremoval of the two protons and precipitation of the CO₂ in stable form.As a further condition of the definition of “CO₂ produced” in thisaspect of the invention, no theoretical or actual calculations ofreduction of the energy load due to, e.g., reuse of byproducts of theprocess for removing the protons (e.g., in the case of the chloralkaliprocess, use of hydrogen produced in the process in a fuel cell or bydirect combustion to produce energy) are included in the total of “CO₂produced.” In addition, no theoretical or actual supplementation of thepower supplied by the power plant with renewable sources of energy isconsidered, e.g., sources of energy that produce little or no carbondioxide, such as wind, solar, tide, hydroelectric, and the like. If theprocess of removing protons includes the use of a hydroxide or otherbase, including a naturally-occurring or stockpiled base, the amount ofCO₂ produced would be the amount that may be stoichiometricallycalculated based on the process by which the base is produced, e.g., forindustrially produced base, the standard chloralkali process or otherprocess by which the base is produced, and for natural base, the besttheoretical model for the natural production of the base.

Using this definition of “CO₂ produced,” in some embodiments theinvention includes forming a stable CO₂-containing precipitate from ahuman-produced gaseous source of CO₂, wherein the formation of theprecipitate utilizes a process for removing protons from an aqueoussolution in which a portion or all of the CO₂ of the gaseous source ofCO₂ is dissolved, and wherein the CO₂ produced by the process ofremoving protons is less than 100, 90, 80, 70, 65, 60, 55, 50, 45, 40,35, 30, 25, 20, 15, 10, or 5% of the CO₂ removed from the gaseous sourceof CO₂ by said formation of precipitate. In some embodiments, theinvention includes forming a stable CO₂-containing precipitate from ahuman-produced gaseous source of CO₂, wherein the formation of theprecipitate utilizes a process for removing protons from an aqueoussolution in which a portion or all of the CO₂ of the gaseous source ofCO₂ is dissolved, and wherein the CO₂ produced by the process ofremoving protons is less than 70% of the CO₂ removed from the gaseoussource of CO₂ by the formation of precipitate. In some embodiments theinvention includes forming a stable CO₂-containing precipitate from ahuman-produced gaseous source of CO₂, wherein the formation of theprecipitate utilizes a process for removing protons from an aqueoussolution in which a portion or all of the CO₂ of the gaseous source ofCO₂ is dissolved, and wherein the CO₂ produced by the process ofremoving protons is less than 50% of the CO₂ removed from the gaseoussource of CO₂ by the formation of precipitate. In some embodiments theinvention includes forming a stable CO₂-containing precipitate from ahuman-produced gaseous source of CO₂, wherein the formation of theprecipitate utilizes a process for removing protons from an aqueoussolution in which a portion or all of the CO₂ of the gaseous source ofCO₂ is dissolved, and wherein the CO₂ produced by the process ofremoving protons is less than 30% of the CO₂ removed from the gaseoussource of CO₂ by the formation of precipitate. In some embodiments, theprocess of removing protons is a process, such as an electrochemicalprocess as described herein, that removes protons without producing abase, e.g., hydroxide. In some embodiments, the process of removingprotons is a process, such as an electrochemical process as describedherein, that removes protons by producing a base, e.g., hydroxide. Insome embodiments, the process is a combination of a process, such as anelectrochemical process as described herein, that removes protonswithout producing a base, e.g., hydroxide, and a process, such as anelectrochemical process as described herein, that removes protons byproducing a base, e.g., hydroxide. In some embodiments, the process ofproton removal comprises an electrochemical process, either removesprotons directly (e.g., direct removal of protons) or indirectly (e.g.,production of hydroxide). In some embodiments a combination ofprocesses, e.g., electrochemical processes is used, where a firstprocess, e.g., electrochemical process, removes protons directly and asecond process, e.g., electrochemical process, removes protonsindirectly (e.g., by production of hydroxide).

In some instances, precipitation of the desired product following CO₂charging (e.g., as described above) occurs without addition of a sourcedivalent metal ions. As such, after the water is charged with CO₂, thewater is not then contacted with a source of divalent metal ions, suchas one or more divalent metal ion salts, e.g., calcium chloride,magnesium chloride, sea salts, etc.

In one embodiment of the invention, a carbonate precipitation processmay be employed to selectively precipitate calcium carbonate materialsfrom the solution in order to provide the desired ratio of magnesium tocalcium, followed by additional CO₂ charging, and in some embodimentsadditional Mg ion charging, and a final carbonate precipitation step.This embodiment is useful in utilizing concentrated waters such asdesalination brine, wherein the cation content is sufficiently high thataddition of more Mg ions is difficult. This embodiment is also useful insolutions of any concentration where two different products are desiredto be produced—a primarily calcium carbonate material, and then amagnesium carbonate dominated material.

The yield of product from a given precipitation reaction may varydepending on a number of factors, including the specific type of wateremployed, whether or not the water is supplemented with divalent metalions, the particular precipitation protocol employed, etc. In someinstances, the precipitation protocols employed to precipitate theproduct are high yield precipitation protocols. In these instances, theamount of product produced from a single precipitation reaction (bywhich is meant a single time that that the water is subjected toprecipitation conditions, such as increasing the pH to a value of 9.5 orhigher, such as 10 or higher as reviewed above in greater detail) may be5 g or more, such as 10 g or more, 15 g or more, 20 g or more, 25 g ormore, 30 g or more, 35 g or more, 40 g or more, 45 g or more, 50 g ormore, 60 g or more, 70 g or more, 80 g or more, 90 g or more, 100 g ormore, 120 g or more, 140 g or more, 160 g or more, 180 g or more, 200 gor more of the storage stable carbon dioxide sequestering product forevery liter of water. In some instances, the amount of product producedfor every liter of water ranges from 5 to 200 g, such as 10 to 100 g,including 20 to 100 g. In instances where the divalent metal ion contentof the water is not supplemented prior to subjecting the water toprecipitate conditions (for example where the water is seawater and theseawater is not supplemented with a source of divalent metal ion orions), the yield of product may range from 5 to 20 g product per literof water, such as 5 to 10, e.g., 6 to 8, g product per liter of water.In other instances where the water is supplemental with a source ofdivalent metal ions, such as magnesium and/or calcium ions, the yield ofproduct may be higher, 2-fold higher, 3-fold higher, 5-fold higher,10-fold higher, 20-fold higher or more, such that the yield of suchprocesses may range in some embodiments from 10 to 200, such as 50 to200 including 100 to 200 g product for every liter of water subjected toprecipitation conditions.

In certain embodiments, a multi-step process is employed. In theseembodiments, a carbonate precipitation process may be employed toselectively precipitate calcium carbonate materials from the solution,followed by additional steps of CO₂ charging and subsequent carbonateprecipitation. The steps of additional CO₂ charging and carbonateprecipitation can in some cases be repeated one, two, three, four, five,six, seven, eight, nine, ten, or more times, precipitating additionalamounts of carbonate material with each cycle. In some cases, the finalpH ranges from about 8 to 10, such as from about 9 to 10, including fromabout 9.5 to 10, for example, from about 9.6 to 9.8.

In certain embodiments, two or more reactors may be used to carry outthe methods described herein. In these embodiments, the method mayinclude a first reactor and a second reactor. In these cases, the firstreactor is used for contacting the initial water with a magnesium ionsource and for charging the initial water with CO₂, as described above.The water may be agitated to facilitate the dissolution of the magnesiumion source and to facilitate contact of the initial water with the CO₂.In some cases, before the CO₂ charged water is transferred to the secondreactor, agitation of the CO₂ charged water is stopped, such thatundissolved solids may settle by gravity. The CO₂ charged water is thentransferred from the first reactor to the second reactor. Aftertransferring the CO₂ charged water to the second reactor, the step ofcarbonate precipitation may be performed, as described herein.

In certain embodiments, a multi-step process, as described above,employing two or more reactors, as described above, can be used to carryout the methods described herein. In these embodiments, a first reactoris used for contacting the initial water with a magnesium ion source andfor charging the initial water with CO₂, as described above.Subsequently, the CO₂ charged water is transferred from the firstreactor to a second reactor for the carbonate precipitation reaction. Incertain embodiments, one or more additional steps of CO₂ charging andsubsequent carbonate precipitation may be performed in the secondreactor, as described above.

In certain embodiments, precipitation conditions can be used that favorthe formation of particular morphologies of carbonate compoundprecipitates. For instance, precipitation conditions can be used thatfavor the formation of amorphous carbonate compound precipitates overthe formation of crystalline carbonate compound precipitates. In thesecases, in addition to contacting the initial water with a magnesium ionsource and charging the initial water with CO₂, as described above, aprecipitation facilitator may be added. In these cases, theprecipitation facilitator facilitates the formation of carbonatecompound precipitates at lower pH's sufficient for nucleation, butinsufficient for crystal formation and growth. Examples of precipitationfacilitators include, but are not limited to, aluminum sulfate(Al₂SO₄)₃. In certain embodiments, the amount of precipitationfacilitator added ranges from about 1 ppm to about 1000 ppm, such asfrom about 1 ppm to about 500, including from about 10 ppm to about 200ppm, for example from about 25 ppm to about 75 ppm. Additionally, the pHof the water can be maintained between about 6 and 8, such as betweenabout 7 and 8, during carbonate compound precipitation formation byalternating CO₂ charging and subsequent carbonate precipitation, asdescribed above.

Alternatively, in yet other embodiments, precipitation conditions can beused that favor the formation of crystalline carbonate compoundprecipitates over the formation of amorphous carbonate compoundprecipitates.

Further details regarding specific precipitation protocols employed incertain embodiments of the invention are provided below with respect tothe description of the figures of the application.

Following production of the precipitate product from the water, acomposition is produced which includes precipitated product and a motherliquor (i.e., the remaining liquid from which the precipitated productwas produced). This composition may be a slurry of the precipitate andmother liquor.

As summarized above, in sequestering carbon dioxide, the precipitatedproduct is disposed of in some manner following its production. Thephrase “disposed of” means that the product is either placed at astorage site or employed for a further use in another product, i.e., amanufactured or man-made item, where it is stored in that other productat least for the expected lifetime of that other product.

In some instances, this disposal step includes forwarding the slurrycomposition described above to a long term storage site. The storagesite could be an above ground site, a below ground site or an underwatersite. In these embodiments, following placement of the slurry at thestorage site, the mother liquor component of the slurry may naturallyseparate from the precipitate, e.g., via evaporation, dispersal, etc.

Where desired, the resultant precipitated product may be separated fromthe resultant mother liquor. Separation of the precipitate can beachieved using any convenient approach. For example, separation may beachieved by drying the precipitated product to produce a driedprecipitated product. Drying protocols of interest include filtering theprecipitate from the mother liquor to produce a filtrate and then airdrying the filtrate. Where the filtrate is air dried, air drying may beat a temperature ranging from −70 to 120° C., as desired. In someinstances, drying may include placing the slurry at a drying site, suchas a tailings pond, and allowing the liquid component of the precipitateto evaporate and leave behind the desired dried product. Also ofinterest are freeze-drying (i.e., lyophilization) protocols, where theprecipitate is frozen, the surrounding pressure is reduced and enoughheat is added to allow the frozen water in the material to sublimedirectly from the frozen precipitate phase to gas. Yet another dryingprotocol of interest is spray drying, where the liquid containing theprecipitate is dried by feeding it through a hot gas, e.g., where theliquid feed is pumped through an atomiser into a main drying chamber anda hot gas is passed as a co-current or counter-current to the atomiserdirection.

Where the precipitated product is separated from the mother liquor, theresultant precipitate may be disposed of in a variety of different ways,as further elaborated below. For example, the precipitate may beemployed as a component of a building material, as reviewed in greaterdetail below. Alternatively, the precipitate may be placed at a longterm storage site (sometimes referred to in the art as a carbon bank),where the site may be above ground site, a below ground site or anunderwater site. Further details regarding disposal protocols ofinterest are provided below.

The resultant mother liquor may also be processed as desired. Forexample, the mother liquor may be returned to the source of the water,e.g., ocean, or to another location. In certain embodiments, the motherliquor may be contacted with a source of CO₂, e.g., as described above,to sequester further CO₂. For example, where the mother liquor is to bereturned to the ocean, the mother liquor may be contacted with a gaseoussource of CO₂ in a manner sufficient to increase the concentration ofcarbonate ion present in the mother liquor. Contact may be conductedusing any convenient protocol, such as those described above. In certainembodiments, the mother liquor has an alkaline pH, and contact with theCO₂ source is carried out in a manner sufficient to reduce the pH to arange between 5 and 9, e.g., 6 and 8.5, including 7.5 to 8.2.

The methods of the invention may be carried out at land or sea, e.g., ata land location where a suitable water is present at or is transportedto the location, or in the ocean or other body ofalkali-earth-metal-containing water, be that body naturally occurring ormanmade. In certain embodiments, a system is employed to perform theabove methods, where such systems include those described below ingreater detail.

The above portion of this application provides an overview of variousaspects of the methods of the invention. Certain embodiments of theinvention are now reviewed further in greater detail in terms of thecertain figures of the invention.

FIG. 1 provides a schematic flow diagram of a carbon dioxidesequestration process that may be implemented in a system, where thesystem may be manifested as a stand-alone plant or as an integrated partof another type of plant, such as a power generation plant, a cementproduction plant, etc. In FIG. 1, water 10 is delivered to aprecipitation reactor 20, e.g., via a pipeline or other convenientmanner, and subjected to carbonate mineral precipitation conditions. Thewater employed in the process illustrated in FIG. 1 is one that includesone or more alkaline earth metals, e.g., calcium, magnesium etc., suchthat it may be viewed as an alkaline-earth-metal-ion-containing water,as reviewed above. In certain embodiments of the invention, the water ofinterest is one that includes calcium in amounts ranging from 50 ppm to20,000 ppm, such as 200 ppm to 5000 ppm and including 400 ppm to 1000ppm. Also of interest are waters that include magnesium in amountsranging from 50 ppm to 40,000 ppm, such as 100 ppm to 10,000 ppm andincluding 500 ppm to 2500 ppm. In embodiments of the invention, thealkaline-earth-metal-ion-containing water is a saltwater. As reviewedabove, saltwaters of interest include a number of different types ofaqueous fluids other than fresh water, such as brackish water, sea waterand brine (including man-made brines, for example geothermal plantwastewaters, desalination waste waters, etc., as well as naturallyoccurring brines as described herein), as well as other salines having asalinity that is greater than that of freshwater. Brine is watersaturated or nearly saturated with salt and has a salinity that is 50ppt (parts per thousand) or greater. Brackish water is water that issaltier than fresh water, but not as salty as seawater, having asalinity ranging from 0.5 to 35 ppt. Seawater is water from a sea orocean and has a salinity ranging from 35 to 50 ppt. Freshwater is waterwhich has a salinity of less than 5 ppt dissolved salts. Saltwaters ofinterest may be obtained from a naturally occurring source, such as asea, ocean, lake, swamp, estuary, lagoon, etc., or a man-made source, asdesired.

As reviewed above, waters of interest also include freshwaters. Incertain embodiments, the water employed in the invention may be amineral rich, e.g., calcium and/or magnesium rich, freshwater source. Insome embodiments, freshwaters, such as calcium rich waters may becombined with magnesium silicate minerals, such as olivine orserpentine, in a solution that has become acidic due to the addition ofcarbon dioxide from carbonic acid, which dissolves the magnesiumsilicate, leading to the formation of calcium magnesium silicatecarbonate compounds. In certain embodiments, the water source can befreshwater wherein metal-ions, e.g., sodium, potassium, calcium,magnesium, etc. are added. Metal-ions can be added to the freshwatersource using any convenient protocol, e.g., as a solid, aqueoussolution, suspension etc.

In certain embodiments, the water may be obtained from the industrialplant that is also providing the gaseous waste stream. For example, inwater cooled industrial plants, such as seawater cooled industrialplants, water that has been employed by the industrial plant may then besent to the precipitation system and employed as the water in theprecipitation reaction. Where desired, the water may be cooled prior toentering the precipitation reactor. Such approaches may be employed,e.g., with once-through cooling systems. For example, a city oragricultural water supply may be employed as a once-through coolingsystem for an industrial plant. The water from the industrial plant maythen be employed in the precipitation protocol, where output water has areduced hardness and greater purity. Where desired, such systems may bemodified to include security measures, e.g., to detect tampering (suchas addition of poisons) and coordinated with governmental agencies,e.g., Homeland Security or other agencies. Additional tampering orattack safeguards may be employed in such embodiments.

As shown in FIG. 1, an industrial plant gaseous waste stream 30 iscontacted with the water at precipitation step 20 to produce a CO₂charged water. By CO₂ charged water is meant water that has had CO₂ gascontacted with it, where CO₂ molecules have combined with watermolecules to produce, e.g., carbonic acid, bicarbonate and carbonateion. Charging water in this step results in an increase in the “CO₂content” of the water, e.g., in the form of carbonic acid, bicarbonateand carbonate ion, and a concomitant decrease in the amount of CO₂ ofthe waste stream that is contacted with the water. The CO₂ charged wateris acidic in some embodiments, having a pH of 6.0 or less, such as 4.0or less and including 3.0 and less. In certain embodiments, the amountof CO₂ of the gas that is used to charge the water decreases by 85% ormore, such as 99% or more as a result of this contact step, such thatthe methods remove 50% or more, such as 75% or more, e.g., 85% or more,including 99% or more of the CO₂ originally present in the gaseous wastestream that is contacted with the water. Contact protocols of interestinclude, but are not limited to: direct contacting protocols, e.g.,bubbling the gas through the volume of water, concurrent contactingmeans, i.e., contact between unidirectionally flowing gaseous and liquidphase streams, countercurrent means, i.e., contact between oppositelyflowing gaseous and liquid phase streams, and the like. The gaseousstream may contact the water source vertically, horizontally, or at someother angle. The CO₂ may be contacted with the water source from one ormore of the following positions: below, above, or at the surface levelof the alkaline-earth-metal-ion-containing water. Contact may beaccomplished through the use of infusers, bubblers, fluidic Venturireactor, sparger, gas filter, spray, tray, catalytic bubble columnreactors, draft-tube type reactors or packed column reactors, and thelike, as may be convenient. Where desired, two or more different CO₂charging reactors (such as columns or other types of reactorconfigurations) may be employed, e.g., in series, such as three or more,four or more, etc. In certain embodiments, various means, e.g.,mechanical stirring, electromagnetic stirring, spinners, shakers,vibrators, blowers, ultrasonication, to agitate or stir the reactionsolution are used to increase the contact between CO₂ and the watersource.

As reviewed above, the gas from the industrial plant 30 may be processedbefore being used to charge the water. For example, the gas may besubjected to oxidation conditions, e.g., to convert CO to CO₂, NO toNO₂, and SO₂ to SO₃, where desired.

At step 20, the storage stable product is precipitated at precipitationstep 20. Precipitation conditions of interest include those thatmodulate the physical environment of the water to produce the desiredprecipitate product. For example, the temperature of the water may beraised to an amount suitable for precipitation of the desired carbonatemineral to occur. In such embodiments, the temperature of the water maybe raised to a value from 5 to 70° C., such as from 20 to 50° C. andincluding 25 to 45° C. As such, while a given set of precipitationconditions may have a temperature ranging from 0 to 100° C., thetemperature may be raised in certain embodiments to produce the desiredprecipitate. In certain embodiments, the temperature is raised usingenergy generated from low- or zero-carbon dioxide emission sources,e.g., solar energy source, wind energy source, hydroelectric energysource, etc. In certain embodiments, excess and/or process heat from theindustrial plant carried in the gaseous waste stream is employed toraise the temperature of the water during precipitation either as hotgases or steam. In certain embodiments, contact of the water with thegaseous waste stream may have raised the water to the desiredtemperature, where in other embodiments, the water may need to be cooledto the desired temperature.

In normal sea water, 93% of the dissolved CO₂ is in the form ofbicarbonate ions (HCO₃ ⁻) and 6% is in the form of carbonate ions (CO₃⁻²). When calcium carbonate precipitates from normal sea water, CO₂ isreleased. In fresh water, above pH 10.33, greater than 90% of thecarbonate is in the form of carbonate ion, and no CO₂ is released duringthe precipitation of calcium carbonate. In sea water this transitionoccurs at a slightly lower pH, closer to a pH of 9.7. While the pH ofthe water employed in methods may range from 5 to 14 during a givenprecipitation process, in certain embodiments the pH is raised toalkaline levels in order to drive the precipitation of carbonatecompounds, as well as other compounds, e.g., hydroxide compounds, asdesired. In certain of these embodiments, the pH is raised to a levelwhich minimizes if not eliminates CO₂ production during precipitation,causing dissolved CO₂, e.g., in the form of carbonate and bicarbonate,to be trapped in the carbonate compound precipitate. In theseembodiments, the pH may be raised to 9 or higher, such as 10 or higher,including 11 or higher.

As summarized above, the pH of the alkaline-earth-metal-ion-containingsource is raised using any convenient approach. In certain embodiments,a pH raising agent may be employed, where examples of such agentsinclude oxides (calcium oxide, magnesium oxide), hydroxides (e.g.,potassium hydroxide, sodium hydroxide, brucite (Mg(OH)₂), etc.),carbonates (e.g., sodium carbonate) and the like.

In embodiments of the invention, ash is employed as a pH modifyingagent, e.g., to increase the pH of the CO₂ charged water. The ash may beused as a as the sole pH modifier or in conjunction with one or moreadditional pH modifiers. Of interest in certain embodiments is use of acoal ash as the ash. The coal ash as employed in this invention refersto the residue produced in power plant boilers or coal burning furnaces,for example, chain grate boilers, cyclone boilers and fluidized bedboilers, from burning pulverized anthracite, lignite, bituminous orsub-bituminous coal. Such coal ash includes fly ash which is the finelydivided coal ash carried from the furnace by exhaust or flue gases; andbottom ash which collects at the base of the furnace as agglomerates.

Fly ashes are generally highly heterogeneous, and include of a mixtureof glassy particles with various identifiable crystalline phases such asquartz, mullite, and various iron oxides. Fly ashes of interest includeType F and Type C fly ash. The Type F and Type C flyashes referred toabove are defined by CSA Standard A23.5 and ASTM C618. The chiefdifference between these classes is the amount of calcium, silica,alumina, and iron content in the ash. The chemical properties of the flyash are largely influenced by the chemical content of the coal burned(i.e., anthracite, bituminous, and lignite). Fly ashes of interestinclude substantial amounts of silica (silicon dioxide, SiO₂) (bothamorphous and crystalline) and lime (calcium oxide, CaO, magnesiumoxide, MgO).

Table 3 below provides the chemical makeup of various types of fly ashthat find use in embodiments of the invention.

TABLE 3 Component Bituminous Subbituminous Lignite SiO₂ (%) 20-60 40-6015-45 Al₂O₃ (%)  5-35 20-30 20-25 Fe₂O₃ (%) 10-40  4-10  4-15 CaO (%) 1-12  5-30 15-40

The burning of harder, older anthracite and bituminous coal typicallyproduces Class F fly ash. Class F fly ash is pozzolanic in nature, andcontains less than 10% lime (CaO). Fly ash produced from the burning ofyounger lignite or subbituminous coal, in addition to having pozzolanicproperties, also has some self-cementing properties. In the presence ofwater, Class C fly ash will harden and gain strength over time. Class Cfly ash generally contains more than 20% lime (CaO). Alkali and sulfate(SO₄) contents are generally higher in Class C fly ashes.

Fly ash material solidifies while suspended in exhaust gases and iscollected using various approaches, e.g., by electrostatic precipitatorsor filter bags. Since the particles solidify while suspended in theexhaust gases, fly ash particles are generally spherical in shape andrange in size from 0.5 μm to 100 μm. Flyashes of interest include thosein which at least about 80%, by weight, comprises particles of less than45 microns. Also of interest in certain embodiments of the invention isthe use of highly alkaline fluidized bed combustor (FBC) fly ash.

Also of interest in embodiments of the invention is the use of bottomash. Bottom ash is formed as agglomerates in coal combustion boilersfrom the combustion of coal. Such combustion boilers may be wet bottomboilers or dry bottom boilers. When produced in a wet or dry bottomboiler, the bottom ash is quenched in water. The quenching results inagglomerates having a size in which 90% fall within the particle sizerange of 0.1 mm to 20 mm, where the bottom ash agglomerates have a widedistribution of agglomerate size within this range. The main chemicalcomponents of a bottom ash are silica and alumina with lesser amounts ofoxides of Fe, Ca, Mg, Mn, Na and K, as well as sulphur and carbon.

Also of interest in certain embodiments is the use of volcanic ash asthe ash. Volcanic ash is made up of small tephra, i.e., bits ofpulverized rock and glass created by volcanic eruptions, less than 2millimeters (0.079 in) in diameter.

In one embodiment of the invention, cement kiln dust (CKD) is added tothe reaction vessel as a means of modifying pH. The nature of the fuelfrom which the ash and/or CKD were produced, and the means of combustionof said fuel, will influence the chemical composition of the resultantash and/or CKD. Thus ash and/or CKD may be used as a portion of themeans for adjusting pH, or the sole means, and a variety of othercomponents may be utilized with specific ashes and/or CKDs, based onchemical composition of the ash and/or CKD.

In embodiments of the invention, ash is added to the reaction as onesource of these additional reactants, to produce carbonate mineralprecipitates which contain one or more components such as amorphoussilica, crystalline silica, calcium silicates, calcium aluminasilicates, or any other moiety which may result from the reaction of ashin the carbonate mineral precipitation process.

The ash employed in the invention may be contacted with the water toachieve the desired pH modification using any convenient protocol, e.g.,by placing an amount of ash into the reactor holding the water, wherethe amount of ash added is sufficient to raise the pH to the desiredlevel, by flowing the water through an amount of the ash, e.g., in theform of a column or bed, etc.

In certain embodiments where the pH is not raised to a level of 12 orhigher, the fly ash employed in the method, e.g., as described below,may not dissolve but instead will remain as a particulate composition.This un-dissolved ash may be separated from the remainder of thereaction product, e.g., filtered out, for a subsequent use.Alternatively, the water may be flowed through an amount of ash that isprovided in an immobilized configuration, e.g., in a column or analogousstructure, which provides for flow through of a liquid through the ashbut does not allow ash solid to flow out of the structure with theliquid. This embodiment does not require separation of un-dissolved ashfrom the product liquid. In yet other embodiments where the pH exceeds12, the ash dissolved and provides for pozzolanic products, e.g., asdescribed in greater detail elsewhere.

In embodiments of the invention where ash is utilized in theprecipitation process, the ash may first be removed from the flue gas bymeans such as electrostatic precipitation, or may be utilized directlyvia the flue gas. The use of ash in embodiments of the invention mayprovide reactants such as alumina or silica in addition to raising thepH.

In certain embodiments of the invention, slag is employed as a pHmodifying agent, e.g., to increase the pH of the CO₂ charged water. Theslag may be used as the sole pH modifier or in conjunction with one ormore additional pH modifiers, e.g., ashes, etc. Slag is generated fromthe processing of metals, and may contain calcium and magnesium oxidesas well as iron, silicon and aluminum compounds. In certain embodiments,the use of slag as a pH modifying material provides additional benefitsvia the introduction of reactive silicon and alumina to the precipitatedproduct. Slags of interest include, but are not limited to, blastfurnace slag from iron smelting, slag from electric-arc or blast furnaceprocessing of steel, copper slag, nickel slag and phosphorus slag.

As indicated above, ash (or slag in certain embodiments) is employed incertain embodiments as the sole way to modify the pH of the water to thedesired level. In yet other embodiments, one or more additional pHmodifying protocols is employed in conjunction with the use of ash.

Alternatively or in conjunction with the use of a pH elevating agent(such as described above), the pH of thealkaline-earth-metal-ion-containing water source can be raised to thedesired level by electrolysis of the water using an electrolytic orelectrochemical protocol. Electrochemical protocols of interest include,but are not limited to, those described above as well as those describedin U.S. Provisional Application Ser. Nos. 61/081,299 and 61/091,729; thedisclosures of which are herein incorporated by reference. Also ofinterest are the electrolytic approaches described in published UnitedStates Application Publication Nos. 20060185985 and 20080248350, as wellas published PCT Application Publication No. WO 2008/018928; thedisclosures of which are hereby incorporated by reference.

Where desired, additives other than pH elevating agents may also beintroduced into the water in order to influence the nature of theprecipitate that is produced. As such, certain embodiments of themethods include providing an additive in the water before or during thetime when the water is subjected to the precipitation conditions.Certain calcium carbonate polymorphs can be favored by trace amounts ofcertain additives. For example, vaterite, a highly unstable polymorph ofCaCO₃ which precipitates in a variety of different morphologies andconverts rapidly to calcite, can be obtained at very high yields byincluding trace amounts of lanthanum as lanthanum chloride in asupersaturated solution of calcium carbonate. Other additives besideslanthanum that are of interest include, but are not limited to,transition metals and the like. For instance, the addition of ferrous orferric iron is known to favor the formation of disordered dolomite(protodolomite) where it would not form otherwise.

The nature of the precipitate can also be influenced by selection ofappropriate major ion ratios. Major ion ratios also have considerableinfluence of polymorph formation. For example, as the magnesium:calciumratio in the water increases, aragonite becomes the favored polymorph ofcalcium carbonate over low-magnesium calcite. At low magnesium:calciumratios, low-magnesium calcite is the preferred polymorph.

Rate of precipitation also has a large effect on compound phaseformation. The most rapid precipitation can be achieved by seeding thesolution with a desired phase. Without seeding, rapid precipitation canbe achieved by rapidly increasing the pH of the sea water, which resultsin more amorphous constituents. When silica is present, the more rapidthe reaction rate, the more silica is incorporated with the carbonateprecipitate. The higher the pH is, the more rapid the precipitation isand the more amorphous the precipitate is.

Accordingly, a set of precipitation conditions to produce a desiredprecipitate from a water include, in certain embodiments, the water'stemperature and pH, and in some instances the concentrations ofadditives and ionic species in the water. Precipitation conditions mayalso include factors such as mixing rate, forms of agitation such asultrasonics, and the presence of seed crystals, catalysts, membranes, orsubstrates. In some embodiments, precipitation conditions includesupersaturated conditions, temperature, pH, and/or concentrationgradients, or cycling or changing any of these parameters. The protocolsemployed to prepare carbonate compound precipitates according to theinvention may be batch or continuous protocols. It will be appreciatedthat precipitation conditions may be different to produce a givenprecipitate in a continuous flow system compared to a batch system.

In certain embodiments, contact between the alkaline-earth-metal-ioncontaining water and CO₂ may be accomplished using any convenientprotocol, (e.g., spray gun, segmented flow-tube reactor) to control therange of sizes of precipitate particles. One or more additives may beadded to the metal-ion containing water source, e.g., flocculants,dispersants, surfactants, antiscalants, crystal growth retarders,sequestration agents etc, in the methods and systems of the claimedinvention in order to control the range of sizes of precipitateparticles.

In the embodiment depicted in FIG. 1, the water from thealkaline-earth-metal-ion-containing water source 10 is first chargedwith CO₂ to produce CO₂ charged water, which CO₂ is then subjected tocarbonate mineral precipitation conditions. As depicted in FIG. 1, a CO₂gaseous stream 30 is contacted with the water at precipitation step 20.The provided gaseous stream 30 is contacted with a suitable water atprecipitation step 20 to produce a CO₂ charged water. By CO₂ chargedwater is meant water that has had CO₂ gas contacted with it, where CO₂molecules have combined with water molecules to produce, e.g., carbonicacid, bicarbonate and carbonate ion. Charging water in this step resultsin an increase in the “CO₂ content” of the water, e.g., in the form ofcarbonic acid, bicarbonate and carbonate ion, and a concomitant decreasein the pCO₂ of the waste stream that is contacted with the water. TheCO₂ charged water can be acidic, having a pH of 6 or less, such as 5 orless and including 4 or less. In some embodiments, the CO₂ charged wateris not acidic, e.g., having a pH of 7 or more, such as a pH of 7-10, or7-9, or 7.5-9.5, or 8-10, or 8-9.5, or 8-9. In certain embodiments, theconcentration of CO₂ of the gas that is used to charge the water is 10%or higher, 25% or higher, including 50% or higher, such as 75% orhigher.

CO₂ charging and carbonate mineral precipitation may occur in the sameor different reactors of the system. As such, charging and precipitationmay occur in the same reactor of a system, e.g., as illustrated in FIG.1 at step 20, according to certain embodiments of the invention. In yetother embodiments of the invention, these two steps may occur inseparate reactors, such that the water is first charged with CO₂ in acharging reactor and the resultant CO₂ charged water is then subjectedto precipitation conditions in a separate reactor. Further reactors maybe used to, e.g., charge the water with desired minerals.

Contact of the water with the source CO₂ may occur before and/or duringthe time when the water is subjected to CO₂ precipitation conditions.Accordingly, embodiments of the invention include methods in which thevolume of water is contacted with a source of CO₂ prior to subjectingthe volume of alkaline-earth-metal-ion-containing water to mineralprecipitation conditions. Embodiments of the invention also includemethods in which the volume of water is contacted with a source of CO₂while the volume of water is being subjected to carbonate compoundprecipitation conditions. Embodiments of the invention include methodsin which the volume of water is contacted with a source of a CO₂ bothprior to subjecting the volume of alkaline-earth-metal-ion-containingwater to carbonate compound precipitation conditions and while thevolume of water is being subjected to carbonate compound precipitationconditions. In some embodiments, the same water may be cycled more thanonce, wherein a first cycle of precipitation removes primarily calciumcarbonate and magnesium carbonate minerals, and leaves remainingalkaline-earth-metal-ion-containing water to which otheralkaline-earth-metal-ion sources may be added, that can have more CO₂cycled through it, precipitating more carbonate compounds.

Regardless of when the CO₂ is contacted with the water, in someinstances when the CO₂ is contacted with the water, the water is notexceedingly alkaline, such that the water contacted with the CO₂ mayhave a pH of 10 or lower, such as 9.5 or lower, including 9 or lower andeven 8 or lower. In some embodiments, the water that is contacted withthe CO₂ is not a water that has first been made basic from anelectrochemical protocol. In some embodiments, the water that iscontacted with the CO₂ is not a water that has been made basic byaddition of hydroxides, such as sodium hydroxide. In some embodiment,the water is one that has been made only slightly alkaline, such as byaddition of an amount of an oxide, such as calcium oxide or magnesiumoxide.

The carbonate mineral precipitation station 20 (i.e., reactor) mayinclude any of a number of different components, such as temperaturecontrol components (e.g., configured to heat the water to a desiredtemperature), chemical additive components, e.g., for introducingchemical pH elevating agents (such as KOH, NaOH) into the water,electrolysis components, e.g., cathodes/anodes, etc, gas chargingcomponents, pressurization components (for example where operating theprotocol under pressurized conditions, such as from 50-800 psi, or100-800 psi, or 400 to 800 psi, or any other suitable pressure range, isdesired) etc, mechanical agitation and physical stirring components andcomponents to re-circulate industrial plant flue gas through theprecipitation plant. The precipitation station 20 may contain componentsthat allow for the monitoring of one or more parameters such as internalreactor pressure, pH, precipitate particle size, metal-ionconcentration, conductivity and alkalinity of the aqueous solution, andpCO₂. Monitoring conditions during the carbonate precipitation processcan allow for corrective adjustments to be made during processing, or ifdesired, to increase or decrease carbonate compound precipitationproduction.

Following production of the storage stable precipitated CO₂ product fromthe water, the resultant precipitated product may be separated from themother liquor to produce separated precipitate product, as illustratedat step 40 of FIG. 1. In some embodiments the precipitate is notseparated, or is only partially separated, from the mother liquor. Insuch embodiments, the mother liquor including some or all of theprecipitate may be disposed of by any suitable means. In someembodiments, the mother liquor including some or all of the precipitateis transported to a land or water location and placed at the location,e.g., the mother liquor including some or all of the precipitate may betransported to the ocean; this is especially useful in embodimentswherein the source of water is seawater. It will be appreciated that thecarbon footprint, amount of energy used, and/or amount of CO₂ producedfor sequestering a given amount of CO₂ from an industrial exhaust gas isminimized in a process where no further processing beyond disposaloccurs with the precipitate. Separation of the precipitate can beachieved using any convenient approach, including a mechanical approach,e.g., where bulk excess water is drained from the precipitate, e.g.,either by gravity alone or with the addition of vacuum, mechanicalpressing (where energy for mechanical pressing can be obtained from theindustrial plant by connecting to the steam turbine, from crushingequipment used to make pulverized coal, etc.) by filtering theprecipitate from the mother liquor to produce a filtrate, etc.Separation can also be achieved by centrifugation or by gravitationalsedimentation of the precipitated product followed by drainage of themother liquor. Separation of bulk water produces a wet dewateredprecipitate.

In the embodiment illustrated in FIG. 1, the resultant dewateredprecipitate is then dried to produce a product, as illustrated at step60 of FIG. 1. Drying can be achieved by air drying the filtrate. Wherethe filtrate is air dried, air drying may be at room or elevatedtemperature. In certain embodiments, the elevated temperature isprovided by the industrial plant gaseous waste stream, as illustrated atstep 70 of FIG. 2. In these embodiments, the gaseous waste stream (e.g.,flue gas) from the power plant may be first used in the drying step,where the gaseous waste stream may have a temperature ranging from 30 to700° C., such as 75 to 300° C. The gaseous waste stream may be contacteddirectly with the wet precipitate in the drying stage, or used toindirectly heat gases (such as air) in the drying stage. The desiredtemperature may be provided in the gaseous waste stream by having thegas conveyer, e.g., duct, from the industrial plant originate at asuitable location, e.g., at a location a certain distance in the HRSG orup the flue, as determined based on the specifics of the exhaust gas andconfiguration of the industrial plant. In yet another embodiment, theprecipitate is spray dried to dry the precipitate, where the liquidcontaining the precipitate is dried by feeding it through a hot gas(such as the gaseous waste stream from the industrial plant), e.g.,where the liquid feed is pumped through an atomizer into a main dryingchamber and hot gas is passed as a co-current or counter-current to theatomizer direction. In certain embodiments, drying is achieved byfreeze-drying (i.e., lyophilization), where the precipitate is frozen,the surrounding pressure is reduced and enough heat is added to allowthe frozen water in the material to sublime directly from the frozenprecipitate phase to gas. Depending on the particular drying protocol ofthe system, the drying station may include a filtration element, freezedrying structure, spray drying structure, etc.

Where desired, the dewatered precipitate product from the separationreactor 40 may be washed before drying, as illustrated at optional step50 of FIG. 1. The precipitate may be washed with freshwater, e.g., toremove salts (such as NaCl) from the dewatered precipitate. Used washwater may be disposed of as convenient, e.g., disposing of it in atailings pond, etc.

In certain embodiments of the invention, the precipitate can beseparated, washed, and dried in the same station for all processes, orin different stations for all processes or any other possiblecombination. For example, in one embodiment, the precipitation andseparation may occur in precipitation reactor 20, but drying and washingoccur in different reactors. In yet another embodiment, precipitation,separation, and drying may occur all in the precipitation reactor 20 andwashing occurring in a different reactor.

Following separation of the precipitate from the mother liquor, e.g., asdescribed above, the separated precipitate may be further processed asdesired. In certain embodiments, the precipitate may then be transportedto a location for long term storage, effectively sequestering CO₂. Forexample, the precipitate may be transported and placed at long termstorage sites, e.g., above ground, below ground, in the deep ocean, etc.as desired.

The dried product may be disposed of in a number of different ways. Incertain embodiments, the precipitate product is transported to alocation for long term storage, effectively sequestering CO₂ in a stableprecipitated product, e.g., as a storage stable above ground CO₂sequestering material. For example, the precipitate may be stored at along term storage site adjacent to the industrial plant andprecipitation system. In yet other embodiments, the precipitate may betransported and placed at long term storage sites, e.g., above ground,below ground, etc. as desired, where the long term storage site isdistal to the power plant (which may be desirable in embodiments wherereal estate is scarce in the vicinity of the power plant). In theseembodiments where the precipitate is transported to a long term storagesite, it may be transported in empty conveyance vehicles (e.g., barges,train cars, trucks, etc.) that were employed to transport the fuel orother materials to the industrial plant and/or precipitation plant. Inthis manner, conveyance vehicles used to bring fuel to the industrialplant, materials to the precipitation plant (e.g., alkali sources) maybe employed to transport precipitated product, and therefore sequesterCO₂ from the industrial plant.

In certain embodiments, the composition is disposed of in an underwaterlocation. Underwater locations may vary depending on a particularapplication. While the underwater location may be an inland underwaterlocation, e.g., in a lake, including a freshwater lake, or interest incertain embodiments are ocean or sea underwater locations. Thecomposition may be still in the mother liquor, without separation orwithout complete separation, or the composition may have been separatedfrom the mother liquor. The underwater location may be shallow or deep.Shallow locations are locations which are 200 feet or less, such as 150feet or less, including 1000 feet or less. Deep locations are thosewhich are 200 feet or more, e.g., 500 feet or more, 1000 feet or more,2000 feet or more, including 5000 feet or more.

Where desired, the compositions made up of the precipitate and themother liquor may be stored for a period of time following precipitationand prior to disposal. For example, the composition may be stored for aperiod of time ranging from 1 to 1000 days or longer, such as 1 to 10days or longer, at a temperature ranging from 1 to 40° C., such as 20 to25° C.

Any convenient protocol for transporting the composition to the site ofdisposal may be employed, and will necessarily vary depending on thelocations of the precipitation reactor and site of disposal relative toeach other, where the site of disposal is an above ground or belowground site disposal, etc. In certain embodiments, a pipeline oranalogous slurry conveyance structure is employed, where theseapproaches may include active pumping, gravitational mediated flow,etc., as desired.

While in certain embodiments the precipitate is directly disposed at thedisposal site without further processing following precipitation, in yetother embodiments the composition may be further processed prior todisposal. For example, in certain embodiments solid physical shapes maybe produced from the composition, where the resultant shapes are thendisposed of at the disposal site of interest. One example of thisembodiment is where artificial reef structures are produced from thecarbonate compound compositions, e.g., by placing the flowablecomposition in a suitable mold structure and allowing the composition tosolidify over time into the desired shape. The resultant solid reefstructures may then be deposited in a suitable ocean location, e.g., ashallow underwater locations, to produce an artificial reef, as desired.

In certain embodiments, the precipitate produced by the methods of theinvention is disposed of by employing it in an article of manufacture.In other words, the product is employed to make a man-made item, i.e., amanufactured item. The product may be employed by itself or combinedwith one or more additional materials, such that it is a component ofthe manufactured items. Manufactured items of interest may vary, whereexamples of manufactured items of interest include building materialsand non-building materials, such as non-cementitious manufactured items.Building materials of interest include components of concrete, such ascement, aggregate (both fine and coarse), supplementary cementitiousmaterials, etc. Building materials of interest also include pre-formedbuilding materials.

Where the product is disposed of by incorporating the product in abuilding material, the CO₂ from the gaseous waste stream of theindustrial plant is effectively sequestered in the built environment.Examples of using the product in a building material include instanceswhere the product is employed as a construction material for some typeof manmade structure, e.g., buildings (both commercial and residential),roads, bridges, levees, dams, and other manmade structures etc. Thebuilding material may be employed as a structure or nonstructuralcomponent of such structures. In such embodiments, the precipitationplant may be co-located with a building products factory.

In certain embodiments, the precipitate product is refined (i.e.,processed) in some manner prior to subsequent use. Refinement asillustrated in step 80 of FIG. 1 may include a variety of differentprotocols. In certain embodiments, the product is subjected tomechanical refinement, e.g., grinding, in order to obtain a product withdesired physical properties, e.g., particle size, etc. In certainembodiments, the precipitate is combined with a hydraulic cement, e.g.,as a supplemental cementitious material, as a sand, a gravel, as anaggregate, etc. In certain embodiments, one or more components may beadded to the precipitate, e.g., where the precipitate is to be employedas a cement, e.g., one or more additives, sands, aggregates,supplemental cementitious materials, etc. to produce final product,e.g., concrete or mortar, 90.

In certain embodiments, the carbonate compound precipitate is utilizedto produce aggregates. Such aggregates, methods for their manufactureand use are described in co-pending United State Application Ser. No.61/056,972 filed May 29, 2008, the disclosure of which is hereinincorporated by reference.

In certain embodiments, the carbonate compound precipitate is employedas a component of hydraulic cement. The term “hydraulic cement” isemployed in its conventional sense to refer to a composition which setsand hardens after combining with water. Setting and hardening of theproduct produced by combination of the cements of the invention with anaqueous fluid result from the production of hydrates that are formedfrom the cement upon reaction with water, where the hydrates areessentially insoluble in water. Such carbonate compound componenthydraulic cements, methods for their manufacture and use are describedin co-pending U.S. application Ser. No. 12/126,776 filed on May 23,2008; the disclosure of which application is herein incorporated byreference.

Also of interest are formed building materials. The formed buildingmaterials of the invention may vary greatly. By “formed” is meantshaped, e.g., molded, cast, cut or otherwise produced, into a man-madestructure defined physical shape, i.e., configuration. Formed buildingmaterials are distinct from amorphous building materials, e.g.,particulate (such as powder) compositions that do not have a defined andstable shape, but instead conform to the container in which they areheld, e.g., a bag or other container. Illustrative formed buildingmaterials include, but are not limited to: bricks; boards; conduits;beams; basins; columns; drywalls etc. Further examples and detailsregarding formed building materials include those described in U.S.Provisional Patent Application Ser. No. 61/110,489 filed on Oct. 31,2008; the disclosure of which is herein incorporated by reference.

Also of interest are non-cementitious manufactured items that includethe product of the invention as a component. Non-cementitiousmanufactured items of the invention may vary greatly. Bynon-cementitious is meant that the compositions are not hydrauliccements. As such, the compositions are not dried compositions that, whencombined with a setting fluid, such as water, set to produce a stableproduct. Illustrative compositions include, but are not limited to:paper products; polymeric products; lubricants; asphalt products;paints; personal care products, such as cosmetics, toothpastes,deodorants, soaps and shampoos; human ingestible products, includingboth liquids and solids; agricultural products, such as soil amendmentproducts and animal feeds; etc. Further examples and detailsnon-cementitious manufactured items include those described in U.S.Provisional Patent Application Ser. No. 61/110,495 filed on Oct. 31,2008; the disclosure of which is herein incorporated by reference.

The resultant mother liquor may also be processed as desired. Forexample, the mother liquor may be returned to the source of the water,e.g., ocean, or to another location. In certain embodiments, the motherliquor may be contacted with a source of CO₂, e.g., as described above,to sequester further CO₂. For example, where the mother liquor is to bereturned to the ocean, the mother liquor may be contacted with a gaseoussource of CO₂ in a manner sufficient to increase the concentration ofcarbonate ion present in the mother liquor. Contact may be conductedusing any convenient protocol, such as those described above. In certainembodiments, the mother liquor has an alkaline pH, and contact with theCO₂ source is carried out in a manner sufficient to reduce the pH to arange between 5 and 9, e.g., 6 and 8.5, including 7.5 to 8.2.Accordingly, the resultant mother liquor of the reaction, e.g., mineralcarbonate depleted water, may be disposed of using any convenientprotocol. In certain embodiments, it may be sent to a tailings pond fordisposal. In certain embodiments, it may be disposed of in a naturallyoccurring body of water, e.g., ocean, sea, lake or river. In certainembodiments, it may be employed as a coolant for the industrial plant,e.g., by a line running between the precipitation system and theindustrial plant. In certain embodiments, it may be employed as greywater, as water input for desalination and subsequent use as freshwater, e.g., in irrigation, for human and animal consumption, etc.Accordingly, of interest are configurations where the precipitationplant is co-located with a desalination plant, such that output waterfrom the precipitation plant is employed as input water for thedesalination plant.

As mentioned above, in certain embodiments the mother liquor produced bythe precipitation process may be employed to cool the power plant, e.g.,in a once through cooling system. In such embodiments, heat picked up inthe process may then be recycled back to precipitation plant for furtheruse, as desired. In such embodiments, the initial water source may comefrom the industrial plant. Such embodiments may be modified to employpumping capacity provided by the industrial plant, e.g., to increaseoverall efficiencies.

Where desired and subsequent to the production of a CO₂ sequesteringproduct, e.g., as described above, the amount of CO₂ sequestered in theproduct is quantified. By “quantified” is meant determining an amount,e.g., in the form of a numeric value, of CO₂ that has been sequestered(i.e., fixed) in the CO₂ sequestering product. The determination may bean absolute quantification of the product where desired, or it may be anapproximate quantification, i.e., not exact. In some embodiments, thequantification is adequate to give a market-acceptable measure of theamount of CO₂ sequestered.

The amount of CO₂ in the CO₂ sequestering product may be quantifiedusing any convenient method. In certain embodiments the quantificationmay be done by actual measurement of the composition. A variety ofdifferent methods may be employed in these embodiments. For example, themass or volume of the composition is measured. In certain embodiments,such measurement can be taken while the precipitate is in the motherliquor. In these cases, additional methods such as x-ray diffraction maybe used to quantify the product. In other embodiments, the measurementis taken after the precipitate has been washed and/or dried. Themeasurement is then used to quantify the amount of CO₂ sequestered inthe product, for example, by mathematical calculation. For example, aCoulometer may be used to obtain a reading of the amount of carbon inthe precipitated sequestration product. This Coulometer reading may beused to determine the amount of alkaline carbonate in the precipitate,which may then be converted into CO₂ sequestered by stoichiometry basedon several factors, such as the initial alkaline metal ion content ofthe water, the limiting reagent of the chemical reaction, thetheoretical yield of the starting materials of the reaction, waters ofhydration of the precipitated products, etc. In some embodiments,contaminants may be present in the product, and other determinations ofthe purity of the product, e.g., elemental analysis, may be necessary todetermine the amount of CO₂ sequestered.

In yet other embodiments, an isotopic method is employed to determinethe carbon content of the product. The ratio of carbon isotopes infossil fuels is substantially different than the ratio of such isotopesin geologic sources such as limestone. Accordingly, the source or ratioof sources of carbon in a sample is readily elucidated via massspectrometry that quantitatively measures isotopic mass. So even iflimestone aggregate is used in concrete (which will increase totalcarbon determined via coulometry), the utilization of mass spectrometryfor isotopic analysis will allow elucidation of the amount of the carbonattributable to captured CO₂ from fossil fuel combustion. In thismanner, the amount of carbon sequestered in the precipitate or even adownstream product that incorporates the precipitate, e.g., concrete,may be determined, particularly where the CO₂ gas employed to make theprecipitate is obtained from combustion of fossil fuels, e.g., coal.Benefits of this isotopic approach include the ability to determinecarbon content of pure precipitate as well as precipitate that has beenincorporated into another product, e.g., as an aggregate or sand in aconcrete, etc.

In other embodiments, the quantification may be done by making atheoretical determination of the amount of CO₂ sequestered, such as bycalculating the amount of CO₂ sequestered. The amount of CO₂ sequesteredmay be calculated by using a known yield of the above described method,such as where the yield is known from previous experimentation. Theknown yield may vary according to a number of factors, including one ormore of the input of gas (e.g. CO₂) and water, the concentration ofalkaline-earth-metal ions in the water, pH, salinity, temperature, therate of the gaseous stream, the embodiment of the method selected, etc.,as reviewed above. Standard information, e.g., a predetermined amount ofCO₂ sequestered per amount of product produced by a given referenceprocess, may be used to readily determine the quantity of CO₂sequestered in a given process that is the same or approximately similarto the reference process, e.g., by determining the amount produced andthen calculating the amount of CO₂ that must be sequestered therein.

Systems of CO₂ Sequestration

Aspects of the invention further include systems, e.g., processingplants or factories, for sequestering CO₂, e.g., by practicing methodsas described above. Systems of the invention may have any configurationwhich enables practice of the particular production method of interest.

FIG. 2 provides a schematic of a system according to one embodiment ofthe invention. In FIG. 2, system 100 includes water source 110. Incertain embodiments, water source 110 includes a structure having aninput for alkaline-earth-metal-ion-containing water, such as a pipe orconduit from an ocean, etc. Where the alkaline-earth-metal-ion watersource that is processed by the system to produce the precipitate isseawater, the input is in fluid communication with a source of seawater, e.g., such as where the input is a pipe line or feed from oceanwater to a land based system or a inlet port in the hull of ship, e.g.,where the system is part of a ship, e.g., in an ocean based system.

Also shown in FIG. 2, is CO₂ source 130. This system also includes apipe, duct, or conduit which directs CO₂ to system 100. The water source110 and the CO₂ gaseous stream source 130 are connected to a CO₂ chargerin precipitation reactor 120. The precipitation reactor 120 may includeany of a number of different design features, such as temperatureregulators (e.g., configured to heat the water to a desiredtemperature), chemical additive components, e.g., for introducingchemical pH elevating agents (such as hydroxides, metal oxides, or flyash) into the water, electrochemical components, e.g., cathodes/anodes,mechanical agitation and physical stirring mechanisms and components tore-circulate industrial plant flue gas through the precipitation plant.Precipitation reactor 120 may also contain design features that allowfor the monitoring of one or more parameters such as internal reactorpressure, pH, precipitate particle size, metal-ion concentration,conductivity and alkalinity of the aqueous solution, and pCO₂. Thisreactor 120 may operate as a batch process or a continuous process.

Precipitation reactor 120, further includes an output conveyance formother liquor. In some embodiments, the output conveyance may beconfigured to transport the mother liquor to a tailings pond fordisposal or in a naturally occurring body of water, e.g., ocean, sea,lake, or river. In other embodiments, the systems may be configured toallow for the mother liquor to be employed as a coolant for anindustrial plant by a line running between the precipitation system andthe industrial plant. In certain embodiments, the precipitation plantmay be co-located with a desalination plant, such that output water fromthe precipitation plant is employed as input water for the desalinationplant. The systems may include a conveyance (i.e., duct) where theoutput water (e.g., mother liquor) may be directly pumped into thedesalination plant.

The system illustrated in FIG. 2 further includes a separator 140 forseparating a precipitated carbonate mineral composition from a motherliquor. In certain embodiments, the separator may achieve separation ofa precipitated carbonate mineral composition from a mother liquor by amechanical approach, e.g., where bulk excess water is drained from theprecipitate by gravity or with the addition of a vacuum, mechanicalpressing, filtering the precipitate from the mother liquor to produce afiltrate, centrifugation or by gravitational sedimentation of theprecipitate and drainage of the mother liquor.

The system also includes a washing station, 150, where bulk dewateredprecipitate from separation station, 140 is washed, e.g., to removesalts and other solutes from the precipitate, prior to drying at thedrying station.

The system further includes a drying station 160 for drying theprecipitated carbonate mineral composition produced by the carbonatemineral precipitation station. Depending on the particular dryingprotocol of the system, the drying station may include a filtrationelement, freeze drying structure, spray drying structure, etc asdescribed more fully above. The system may include a conveyer, e.g.,duct, from the industrial plant that is connected to the dryer so that agaseous waste stream (i.e., industrial plant flue gas) may be contacteddirectly with the wet precipitate in the drying stage.

The dried precipitate may undergo further processing, e.g., grinding,milling, in refining station, 180, in order to obtain desired physicalproperties. One or more components may be added to the precipitate wherethe precipitate is used as a building material.

The system further includes outlet conveyers, e.g., conveyer belt,slurry pump, that allow for the removal of precipitate from one or moreof the following: the reactor, drying station, washing station or fromthe refining station. The product of the precipitation reaction may bedisposed of in a number of different ways. The precipitate may betransported to a long term storage site in empty conveyance vehicles,e.g., barges, train cars, trucks, etc., that may include both aboveground and underground storage facilities. In other embodiments, theprecipitate may be disposed of in an underwater location. Any convenientprotocol for transporting the composition to the site of disposal may beemployed. In certain embodiments, a pipeline or analogous slurryconveyance structure may be employed, where these approaches may includeactive pumping, gravitational mediated flow, etc.

In certain embodiments, the system will further include a station forpreparing a building material, such as cement, from the precipitate.This station can be configured to produce a variety of cements,aggregates, or cementitious materials from the precipitate, e.g., asdescribed in co-pending U.S. application Ser. No. 12/126,776; thedisclosure of which application is herein incorporated by reference.

As indicated above, the system may be present on land or sea. Forexample, the system may be a land based system that is in a coastalregion, e.g., close to a source of sea water, or even an interiorlocation, where water is piped into the system from a salt water source,e.g., ocean. Alternatively, the system may be a water based system,i.e., a system that is present on or in water. Such a system may bepresent on a boat, ocean based platform etc., as desired. In certainembodiments, the system may be co-located with an industrial plant atany convenient location. The precipitation plant may be a land-basedplant that is co-located with the land-based industrial plant, e.g., ina coastal region, such as close to a source of analkaline-earth-metal-ion-containing water, e.g., seawater. Also ofinterest are interior locations, where water is piped into the systemdirectly from a water source, e.g., the industrial plant, a distal lake,a distal ocean. Alternatively, the precipitation plant may be present onwater, e.g., on a barge, boat, ocean based platform etc., as desired,for example where real-estate next to a industrial plant is scarce. Incertain embodiments, the precipitation plant may be a mobile plant, suchthat it is readily co-located with an industrial plant.

Systems of the invention that are co-located with an industrial plant,such as a power plant, may be configured to allow for synchronizing theactivities of the industrial plant and precipitation plant. In certaininstances, the activity of one plant may not be matched to the activityof the other. For example, the precipitation plant may need to reduce orstop its acceptance of the gaseous waste stream but the industrial plantmay need to keep operating. Conversely, situations may arise where theindustrial plant reduces or ceases operation and the precipitation plantdoes not. To address situations where either the precipitation plant orindustrial plant may need to reduce or stop its activities, designfeatures that provide for continued operation of one of the co-locatedplants while the other reduces or ceases operation may be employed, asdescribed in detail above. For example, the systems of the invention mayinclude in certain embodiments, blowers, fans, and/or compressors atvarious points along the connecting line between the industrial plantand the precipitation plant in order to control the occurrence ofbackpressure in the ducts that connect the industrial plant to theprecipitation plant. In certain embodiments, a gas storage facility maybe present between the industrial plant and the precipitation plant.Where desired, the precipitation plant may include emissions monitors toevaluate any gaseous emissions produced by the precipitation plant asrequired by Air Quality Agencies.

Aspects of the invention include the use of a CO₂ containing industrialplant gaseous waste stream, e.g., an industrial plant flue gas, at oneor more stages of a process in which a storage stable CO₂ containingproduct is precipitated. As such, the CO₂ containing industrial plantgaseous waste stream is employed in a precipitation process. Inembodiments of the invention, the gaseous waste stream is employed atone or more steps of the precipitation process, such as in aprecipitation step, e.g., where it is employed to charge water with CO₂,or during a precipitate drying step, e.g., where precipitated carbonatecompound is dried, etc. Where desired, the flue gas from the industrialplant can be re-circulated through the precipitation plant until totaladsorption of the remnant CO₂ approaches 100%, or a point of diminishingreturns is achieved such that the remaining flue gas can be processedusing alternative protocols and/or released into the atmosphere.

As reviewed above, precipitation systems of the invention may beco-located with an industrial plant. An example of such a system isillustrated in FIG. 2. In FIG. 2, flue gas outlet 170 from power plant200 is used in both the precipitation reactor 120 as the source of CO₂130 and the dryer 160 and the source of heat. Where desired,backpressure controls are employed to at least reduce, if not eliminate,the occurrence of backpressure which could arise from directing aportion of, if not all of, the industrial plant gaseous waste stream tothe precipitation plant 100. Any convenient manner of controllingbackpressure occurrence may be employed. In certain embodiments,blowers, fans and/or compressors are provided at some point along theconnecting line between the industrial plant and precipitation plant. Incertain embodiments, the blowers are installed to pull the flue gas intoducts that port the flue gas to the precipitation plant. The blowersemployed in these embodiments may be electrically or mechanically drivenblowers. In these embodiments, if present at all, backpressure isreduced to a level of 5 inches or less, such as one inch or less. Incertain embodiments, a gas storage facility may be present between theindustrial plant and the precipitation plant. When present, the gasstorage facility may be employed as a surge, shutdown and smoothingsystem so that there is an even flow of flue gases to the precipitationplant.

Aspects of the invention include synchronizing the activities of theindustrial plant and precipitation plant. In certain instances, theactivity of one plant may not be matched to the activity of the other.For example, the precipitation plant may need to reduce or stop itsacceptance of the gaseous waste stream but the industrial plant may needto keep operating. Conversely, situations may arise where the industrialplant reduces or ceases operation and yet the precipitation plant doesnot. To address such situations, the plants may be configured to providefor continued operation of one of the co-located plants while the otherreduces or ceases operation may be employed. For example, to address thesituation where the precipitation plant has to reduce or eliminate theamount of gaseous waste stream it accepts from the industrial plant, thesystem may be configured so that the blowers and ducts conveying wastestream to the precipitation plant shut off in a controlled sequence tominimize pressure swings and the industrial plant flue acts as a bypassstack for discharge of the gaseous waste stream. Similarly, if theindustrial plant reduces or eliminates its production of gaseous wastestream, e.g., the industrial plant is dispatched wholly or partiallydown, or there is curtailment of industrial plant output under somepre-agreed level, the system may be configured to allow theprecipitation plant to continue operation, e.g., by providing analternate source of CO₂, by providing for alternate heating protocols inthe dryer, etc.

Where desired, the precipitation plant may include emissions monitors toevaluate any gaseous emissions produced by the precipitation plant andto make required reports to regulatory agencies, both electronic(typically every 15 minutes), and daily, weekly, monthly, quarterly, andannually. In certain embodiments, gaseous handling at the precipitationplant is sufficiently closed that exhaust air from the precipitationplant which contains essentially all of the unused flue gas from theindustrial plant is directed to a stack so that required ContinuousEmissions Monitoring Systems can be installed in accordance with thestatutory and regulatory requirements of the Country, province, statecity or other political jurisdiction.

In certain embodiments, the gaseous waste stream generated by theindustrial plant and conveyed to the precipitation plant has beentreated as required by Air Quality Agencies, so the flue gas deliveredto the precipitation plant already meets Air Quality requirements. Inthese embodiments, the precipitation plant may or may not havealternative treatment systems in place in the event of a shutdown of theprecipitation plant. However, if the flue gas delivered to has been onlypartially treated or not treated at all, the precipitation plant mayinclude air pollution control devices to meet regulatory requirements,or seek regulatory authority to emit partially-treated flue gas forshort periods of time. In yet other embodiments, the flue gas isdelivered to precipitation plant for all processing. In suchembodiments, the system may include a safeguard for the situation wherethe precipitation plant cannot accept the waste stream, e.g., byensuring that the pollution controls installed in the industrial plantturn on and control emissions as required by the Air Quality Agencies.

The precipitation plant that is co-located with the industrial plant maybe present at any convenient location, be that on land or water. Forexample, the precipitation plant may be a land-based plant that isco-located with the land-based industrial plant, e.g., in a coastalregion, such as close to a source of sea water. Also of interest areinterior locations, where water is piped into the system directly from awater source, e.g., the industrial plant, a distal lake, a distal ocean.Alternatively, the precipitation plant may be present on water, e.g., ona barge, boat, ocean based platform etc., as desired, for example wherereal-estate next to a industrial plant is scarce. In certainembodiments, the precipitation plant may be a mobile plant, such that itis readily co-located with an industrial plant.

As indicated above, of interest in certain embodiments are waste streamsproduced by integrated gasification combined cycle (IGCC) plants. Inthese types of plants, the initial fuel, e.g., coal, biomass, etc., isfirst subjected to a gasification process to produce syngas, which maybe shifted, generating amounts of CO₂, CO and H₂. The product of thegasification protocol may be conveyed to the precipitation plant tofirst remove CO₂, with the resultant CO₂ scrubbed product being returnedto a power plant for use as fuel. In such embodiments, a line from thegasification unit of a power plant may be present between a power plantand precipitation plant, and a second return line may be present betweenthe precipitation plant and a power plant to convey scrubbed syngas backto a power plant.

In certain embodiments, the co-located industrial plant andprecipitation plant (or integrated plant) is operated with additionalCO₂ emission reduction approaches. For example, material handling,vehicles and earthmoving equipment, locomotives, may be configured touse biofuels in lieu of fossil fuels. In such embodiments, the site mayinclude fuel tanks to store the biofuels

In addition to sequestering CO₂, embodiments of the invention alsosequester other components of industrial plant generated gaseous wastestreams. For example, embodiments of the invention results insequestration of at least a portion of one or more of NOx, SOx, VOC,Mercury and particulates that may be present in the waste stream, suchthat one or more of these products are fixed in the solid precipitateproduct.

In FIG. 2, precipitation system 100 is co-located with industrial plant200. However, precipitation system 100 is not integrated with theindustrial plant 200. Of further interest in certain embodimentstherefore is an integrated facility which, in addition to an industrialplant, includes power generation, water treatment (seawaterdesalinization or mineral rich freshwater treatment) and precipitationcomponents as described in U.S. patent application Ser. No. 12/163,205,the disclosure of which is herein incorporated by reference. The watersource for the precipitation plant may be derived from the waste streamsof the water treatment plant. The resultant mother liquor from thecarbonate precipitation plant may be used as the feedstock for the watertreatment plant. The resultant integrated facility essentially usesfuel, minerals and untreated water as inputs, and outputs energy, aprocessed industrial product, e.g., cement, clean water, clean air andcarbon-sequestering building materials.

FIG. 3 provides an example of where a precipitation system 100 isintegrated with an industrial plant, in this case a coal fired powerplant 300. In power plant 300, coal 310 fuels steam boiler 315 toproduce steam which in turn runs a turbine (not shown) to produce power.Steam boiler 315 also produces bottom ash or boiler slag 325 and fluegas 320. Flue gas 320 contains fly ash, CO₂ and sulfates. Flue gas 320and bottom ash 325 are combined with water from water source 330 inreactor 340 and subjected to precipitation reactions, as describedabove. Pump 350 facilitates transport of precipitated product fromreactor 340 to spray dryer 360, which employs flue gas 320 to spray drythe precipitated product for subsequent disposal, e.g., by placement ina landfill or use in a building product. Treated flue gas 370 exitsspray dryer 360 and then is discharged to the atmosphere in stack 380.Treated flue gas 370 is gas in which the fly ash, sulfur, and CO₂content has been substantially reduced, if not completely removed, ascompared to flue gas 320. As an example of the system shown in FIG. 3,the CO₂ source may be flue gas from coal or other fuel combustion, whichis contacted with the volume of saltwater with little or no pretreatmentof the flue gas. In these embodiments, the use of fuels such ashigh-sulfur coal, sub-bituminous coal, lignite and the like, which areoften inexpensive and considered low quality, is practical due to theability of the process to remove the SOx and other pollutants as well asremoving CO₂. These fuels may also provide higher levels of co-reactantssuch as alumina and silica in fly ash carried by the flue gas, producingmodified carbonate mineral precipitates with beneficial properties.

When co-located with a power plant, methods of the invention providesequestration of substantial amounts of CO₂ from the gaseous wastestream produced by the power plant with a limited parasitic energyrequirement. In some instances, the methods provide for removal of 5% ormore, 10% or more, 25% or more, 50% or more, 75% or more of the CO₂ fromthe gaseous waste stream with a parasitic energy requirement of 50% orless, such as 30% or less, including 25% or less. The parasitic energyrequirement is the amount of energy generated by the power plant that isrequired to operate the carbon dioxide sequestration process. In someinstances the above levels of CO₂ removal are achieve with a parasiticenergy requirement of 20% or less, 15% or less, 10% or less.

Another type of industrial plant which may be co-located with aprecipitation plant of the invention is a cement plant, such as aportland cement production plant. FIG. 4 provides a schematic of anexemplary portland cement production facility. In FIG. 4, limestone 400along with shales and other additives 410 are milled to appropriate sizeand moved through precalciner 500, which uses waste heat from flue gas430 to preheat the mixture, utilizing waste heat from kiln 510 toimprove operational efficiency. The preheated mixture enters kiln 510where it is further heated by burning coal 420. The resultant clinker480 is collected and stored in silos 570, where it is blended withadditives 571 such as gypsum, limestone, etc. and ground to desired sizein ball mill 580. The product which exits the ball mill is portlandcement 490 which is stored in cement silo 590 prior to shipment tocustomers.

The flue gas 430 which comes from kiln 510 contains both gaseous andparticulate contaminants. The particulate contaminants are known as kilndust 440, and are removed from the flue gas via electrostaticprecipitators or baghouses 520. The kiln dust so removed is commonlysent to landfill 600, though occasionally kiln dust is recycled into thekiln, or sold as a supplementary cementitious material. The flue gas isthen pulled by fan 540 into wet scrubber 550, where the sulfur oxides inthe flue gas are removed by reaction with a calcined lime slurry,producing a calcium sulfite (e.g., gypsum) slurry 480 which is normallydewatered in reclaim tank 572 and disposed of in landfill 600. The fluegas 430 exits wet scrubber 430 and is released to the atmosphere viastack 560. The flue gas so released has a high concentration of CO₂,which is released both by the burning of coal and via the calcinationrequired to oxidize limestone to portland cement.

FIG. 5 shows a schematic of an exemplary co-located cement plant andprecipitation plant according to one embodiment of the invention. Theprocess in this example is the same as that in FIG. 4, except that acarbonate precipitation plant replaces the flue gas treatment system ofFIG. 4. Once the flue gas exits the precalciner 500, it is pulled by fan540 to reactor 630, wherein a precipitation reaction is initiatedutilizing seawater 620 and alkali 625. The resultant slurry 631 ispumped via pump 640 to drying station 650, where water 651 is dischargedand dried cementitious material 660 is stored for shipment to customers.Flue gas 430 is emitted from stack 670 with a portion if not all of thecontaminants removed, including mercury, SO_(x), particulates, and CO₂.

FIG. 5 shows a schematic of an exemplary cement plant which does notrequire a limestone quarry, according to one embodiment of theinvention. In this embodiment, the product of reactor 630 may take theform of a relatively pure calcium carbonate during portions of timeduring its operation, and other forms of building materials during otherportions of time. In this example, rather than mined limestone, theprecalciner 500 and kiln 510 is charged with a mixture of shale andother ingredients 410 blended with a relatively pure precipitatedcalcium carbonate 670. Previously mentioned and incorporated byreference U.S. patent application Ser. No. 12/126,776 details protocolsof precipitating an aragonite calcium carbonate from seawater using fluegas. By using the product of the flue gas treatment reactor as afeedstock, the cement plant draws its calcium ion from the sea via theprecipitated product, and only requires mined limestone in the firstshort period of operation until sufficient precipitated calciumcarbonate is generated to charge the kiln.

In embodiments of the invention, the carbonate precipitation isperformed in two stages. The first stage selectively precipitatescalcium carbonate, which can then be used as a feedstock for the cementplant as illustrated in FIG. 6. The second precipitation stage canproduce a number of different materials, including cements, aggregates,above ground carbon sequestering materials, and the like.

Portland cement is 60-70% by mass CaO, which is produced by heatingCaCO₃, requiring heat and releasing one molecule of CO₂ for everymolecule of CaO released. Because of the additional CO₂ released fromthe burning of fuel, the output of precipitated CaCO₃ from theprecipitation plant will exceed the amount required to provide feedstockfor the cement plant. In this instance a portion of the time ofoperation of the precipitation plant may be devoted to production ofother cementitious materials 660 such as those described in U.S.application Ser. No. 12/126,776; the disclosures of which are hereinincorporated by reference.

The portland cement 490 produced as shown in FIG. 6 is carbon neutral asthe CO₂ from its manufacture is sequestered into precipitated carbonatemineral 670 and cementitious materials 660. The portland cement 490 maybe sold as is, or blended or interground with cementitious material 660to produce a blended cement.

An example of a continuous feed system of interest is depicted in FIG.11. In FIG. 11, system 1100 includes water source (e.g., pipe from oceanto provide seawater) 1101 which is in fluid communication with reactor1110. Also present in reactor 1110 is Ca/Mg/OH ion sources and catalysts1111, which have been added in amounts sufficient to raise the Mg/Ca ionratio in water present in reactor 1110 to 3 or more. Reactor 1110 mayconfigured as a packed bed column, and configured from bicarbonatecharging, if desired. CO₂ containing gas, e.g., flue gas 1112, iscombined with water in reactor 1110 by sparger/bubbler 1113. The Mg ionsource and CO₂ are combined with the water in reactor 1110 to produceCO₂ charged acidic water, which flows out of reactor 1110 at a pH ofbetween 4.8 and 7.5. Next, the CO₂ charged acidic water flows throughconduit 1120 where it is cycled through different levels of alkalinity,e.g., 8.5 and 9.8, with the use of various CO₂ gas injectors 1121, OH—modulators 1123 (such as introduces pH elevating agents, and includeselectrodes, etc.) and static mixers 1122 positioned at various locationsalong conduit 1120. The flow rate through conduit 1120 may be controlledas desired, e.g., to be between 1 GPM and 1,000,000 GPM, such as 30 GPMand 100,000 GPM and including 4,000 GPM and 60,000 GPM. The length ofconduit 1120 may vary, ranging from 100 ft to 20,000 ft, such as 1000 ftto 7000 ft. At the end of conduit 1120, as slurry product 1130 isobtained, which slurry product includes the precipitated CO₂sequestering product and mother liquor. The resultant slurry is thenforwarded to a water/solids separator or settling tank, as illustratedat 1140.

In certain embodiments, two or more reactors may be used to carry outthe methods described herein. A schematic of an embodiment using tworeactors is shown in FIGS. 12A, 12B, and 12C. In this embodiment, themethod may include a first reactor 1210 and a second reactor 1220. Inthese cases, the first reactor 1210 is used for contacting the initialwater, e.g. fresh seawater 1230, with a magnesium ion source 1240 andfor charging the initial water with CO₂ containing gas, e.g. flue gas1250 (where this step is also referred to as bicarbonate charging). Theflue gas 1250 may be contacted with the water in the first reactor 1210through a sparger/bubbler 1280. The water is agitated with agitator 1260to facilitate the dissolution of the magnesium ion source and tofacilitate contact of the initial water with the CO₂ containing gas. Insome cases, before the CO₂ charged acidic water is transferred to thesecond reactor 1220, agitation of the CO₂ charged acidic water isstopped, such that undissolved solids may settle by gravity. The CO₂charged acidic water is then transferred through conduit 1270 from thefirst reactor 1210 to the second reactor 1220.

After transferring the CO₂ charged acidic water to the second reactor1220, the step of carbonate precipitation may be performed. In somecases, a pH raising agent 1290 is contacted with the water in the secondreactor 1220 to facilitate formation of the carbonate containingprecipitate. The contents of the second reactor 1220 may be agitatedwith agitator 1295. In certain embodiments, one or more additional stepsof CO₂ charging and subsequent carbonate precipitation may be performedin the second reactor, as described above. In these cases, additionalCO₂ containing gas, e.g. flue gas 1255, is contacted with the water inthe second reactor 520 through sparger/bubbler 1285. The resultingslurry product includes the precipitated CO₂ sequestering product andmother liquor, which is then forwarded to a water/solids separator orsettling tank, as described above.

The following examples are put forth so as to provide those of ordinaryskill in the art with a complete disclosure and description of how tomake and use the present invention, and are not intended to limit thescope of what the inventors regard as their invention nor are theyintended to represent that the experiments below are all or the onlyexperiments performed. Efforts have been made to ensure accuracy withrespect to numbers used (e.g. amounts, temperature, etc.) but someexperimental errors and deviations should be accounted for. Unlessindicated otherwise, parts are parts by weight, molecular weight isweight average molecular weight, temperature is in degrees Centigrade,and pressure is at or near atmospheric.

EXPERIMENTAL Example I Precipitation of P00099

A. P00099 Precipitation Process

The following protocol was used to produce the P00099 precipitate. 380 Lof filtered seawater was pumped into a cylindrical polyethylene 60°-conebottom graduated tank. This reaction tank was an open system, leftexposed to the ambient atmosphere. The reaction tank was constantlystirred using an overhead mixer. pH, room temperature, and watertemperature were constantly monitored throughout the reaction.

25 g of granulated (Ca,Mg)O (a.k.a., dolime or calcined dolomite) wasmixed into the seawater. Dolime that settled to the bottom of the tankwas manually re-circulated from the bottom of the tank through the topagain, in order to facilitate adequate mixing and dissolution ofreactants. A second addition of 25 g of dolime was performed in anidentical manner, including a manual recirculation of settled reactant.When the pH of the water reached 9.2, a gas mixture of 10% CO₂ (and 90%compressed air) was slowly diffused through a ceramic airstone intosolution. When the pH of the solution fell to 9.0, another 25 g additionof dolime was added to the reaction tank, which caused the pH to riseagain. The additions of dolime were repeated whenever the pH of thesolution dropped to 9.0 (or below), until a total of 225 g were added. Amanual recirculation of settled reactant was performed in between eachdolime addition.

After the final addition of dolime, the continuous diffusion of gasthrough the solution was stopped. The reaction was stirred for anadditional 2 hours. During this time, the pH continued to rise. Tomaintain a pH between 9.0 and 9.2, additional gas was diffused throughthe reaction when the pH rose above 9.2 until it reached 9.0. Manualre-circulations of settled reactant were also performed 4 timesthroughout this 2 hour period.

2 hours after the final addition of dolime, stirring, gas diffusion andrecirculation of settled reactant was stopped. The reaction tank wasleft undisturbed for 15 hours (open to the atmosphere).

After the 15 hour period, supernatant was removed through the top of thereaction tank using a submersible pump. The remaining mixture wasremoved through the bottom of the tank. The collected mixture wasallowed to settle for 2 hours. After settling, the supernatant wasdecanted. The remaining slurry was vacuum filtered through 11 μm poresize filter paper, in a Büchner funnel. The collected filter cake wasplaced into a Pyrex dish and baked at 110° C. for 24 hours.

The dried product was ground in a ball mix and fractioned by sizethrough a series of sieves to produce the P00099 precipitate.

B. Materials Analysis

Of the different sieve fractions collected, only the fraction containingparticles retained on the 38 μm-opening sieve and passing through the 75μm-opening sieve was used.

1. Chemical Characteristics

The P00099 precipitate used for the blend was analyzed for elementalcomposition using XRF. Results for the main elements are reported forthe QUIKRETE™ type I/II Portland cement used in this blend as well asfor the P00099 precipitate. In Table 4, below.

TABLE 4 Table 4: XRF analysis of the type I/II portland cement andP00099-002 used in this blend P₂O₅ Sr CO₃ % Sample Na₂O % MgO % Al₂O₃ %SiO₂ % ppm SO₃ % Cl % K₂O % CaO % Fe₂O₃ % ppm diff. OPC1 2.15 1.95 4.3220.31 2336 2.54 0.072 0.36 62.88 3.88 1099 0.002 P00099 1.36 3.44 0.140.083 462 0.65 1.123 0.04 45.75 0.12 3589 46.82The XRD analysis of this precipitate indicates the presence of aragoniteand magnesium calcite (composition close to Mg_(0.1)Ca_(0.9)CO₃) and inminor amounts, brucite and halite (Table 5). The FT-IR analysis of theP00099 precipitate confirmed the presence of aragonite, calcite andbrucite.

TABLE 5 Magnesium Sample Aragonite Calcite Brucite Halite P00099 79.917.1 2.8 0.2The total inorganic carbon content measured by coulometry is in fairagreement with the same value derived from the XRD Rietveld estimatedcomposition coupled with XRF elemental composition. Table 6 provides acoulometric analysis of P00099 compared to % C derived from XRD/XRFdata.

TABLE 6 Total C derived from other analytical Total C from coulometrydata 10.93 ± 0.16% 11.5%2. Physical Characteristics

SEM observations on the precipitate confirmed the dominance of aragonite(needle-like) as well as the size of the particle agglomerates. Thedetermined BET specific surface areas (“SSA”) of the Portland cement andthe P00099 precipitate are given in Table 7.

TABLE 7 Type I/II Quikrete Portland cement P00099 1.18 ± 0.04 m²/g 8.31± 0.04 m²/g

The particle size distribution was determined after 2 minutes ofpre-sonication to dissociate the agglomerated particles.

Example II Use of Fly Ash as an Alakali Source

A. Methods

500 mL of seawater (initial pH=8.01) was continuously stirred in a glassbeaker using a magnetic stir bar. The pH and temperature of the reactionwas continuously monitored. Class F fly ash (˜10% CaO) was incrementallyadded as a powder, allowing the pH to equilibrate in between additions.

B. Results and Observations:

(Amounts of fly ash listed are the cumulative totals, i.e. the totalamount added at that point in the experiment.)

After the additions of 5.00 g of fly ash the pH reached 9.00.

34.14 g-->9.50

168.89 g-->9.76

219.47 g-->10.94

254.13 g-->11.20

300.87 g-->11.28

Much more fly ash was needed to raise the pH of the seawater thandistilled water.

The initial pH raise (8 to 9) required much less fly ash than thefurther raises. The pH remained fairly stable around 9.7 for much of thereaction. The rate of rate of pH increase went up after ˜10. Also ofnote was an initial drop in pH when the fly ash was added. This drop inpH is quickly overcome by the effects of the calcium hydroxide. SEMimages of vacuum dried slurry from the reaction showed some spheres ofthe fly ash that had partially dissolved. The remaining spheres alsoseemed to be embedded in a possibly cementitious material.

C. Conclusions

In fresh (distilled) water, it was found that small amounts of class Ffly ash (<1 g/L) immediately raised the pH from 7 (neutral) to ˜11. Thesmall amount necessary to raise the pH is most likely due to theunbuffered nature of nature of distilled water. Seawater is highlybuffered by the carbonate system, and thus it took much more fly ash toraise the pH to similar levels.

Example III Production of High Yields

A. Process 1

A 20% CO₂/80% Air gas mixture was sparged into 1 L of seawater until apH<5 was reached. Once reached, 1.0 g of Mg(OH)₂ was added to the 1 L ofcarbonic acid/seawater solution. The 20/80 gas mixture continued to besparged for 20 minutes to ensure maximal dissolution of the Mg(OH)₂ andgases. After dissolution, sparging was stopped and 2M NaOH was addeduntil a pH of 9.8 was reached. Sparging of the 20/80 gas was resumeduntil a pH of 8.5 was reached. 2M NaOH and counter-additions of the20/80 gas were continued maintaining a pH range between 8.5 and 9.8until a total of 200 ml of 2M NaOH was added. A yield of 6.91 g wasobserved having a Coulometer reading of 10.6% carbon (˜80% carbonate).

B. Process 2

A 20% CO₂/80% Air gas mixture was sparged into 1 L of seawater until apH<5 was reached. Once reached, 2.69 g of Mg(OH)₂ was added to the 1 Lof carbonic acid/seawater solution. The 20/80 gas mixture continued tobe sparged for 20 minutes to ensure maximal dissolution of the Mg(OH)₂and gases. After dissolution, sparging was stopped and 2M NaOH was addeduntil a pH of 9.8 was reached. Sparging of the 20/80 gas was resumeduntil a pH of 8.5 was reached. 2M NaOH and counter-additions of the20/80 gas were continued maintaining a pH range between 8.5 and 9.8until a total of 200 ml of 2M NaOH was added. A yield of 10.24 g wasobserved having a Coulometer reading of 9.7% carbon (˜75% carbonate).

SEM, EDS, and X-Ray Diffraction of the precipitated carbonates showedamorphous and crystalline Ca and Mg carbonates, and also the presence ofCa/Mg carbonates. Pictures of the precipitates are provided in FIGS. 13Aand 13B.

C. Process 3

CO₂ was sparged into 1 L seawater until a pH 7 or lower was reached. 0to 5.0 g Mg ion supplement referred to as “Moss Mag” and obtained fromCalera Corporation's Moss Landing site (which is the former site of theKaiser Aluminum & Chemical Corporation and National Refractorie in MossLanding Calif., where the supplement is Mg rich waste product found intailings ponds of the site) was added while mixing and continuing tosparge CO₂. 0.175 ppm Al₂(SO₄)₃ was added. CO₂ was continued to besparged and base was added while maintaining a pH between 7 and 8 endingat a pH of 7. Sparging of CO₂ was stopped and base was added until a pHbetween 9.0 and 10.4 was reached. As shown in FIG. 14, the abovereaction conditions favour the formation of amorphous carbonate compoundprecipitates. The resultant amorphous precipitate product is readilyspray dried to produce a dry product.

D. Process 4

As shown in FIGS. 12A, 12B and 12C, in certain embodiments, amulti-step, multi-reactor process is used to carry out the methodsdisclosed herein. In the first reactor, a magnesium ion source obtainedfrom a Moss Landing, Calif. site (hereinafter referred to as Moss Mag),was put into solution using carbonic acid and agitation. The pH of theseawater in the first reactor was maintained a pH of 7.0 or less duringMoss Mag dissolution. In certain embodiments, 1.0 gram of 50-150 μm MossMag was dissolved into solution per 1 L of seawater. A pH of 6.2-6.6 ora hardness reading>0.08 grams/liter indicated that the appropriateamount of Moss Mag was dissolved in solution. A source of CO₂, e.g. fluegas, was sparged into the water in the first reactor. About 40-50% ofthe total flue gas consumed during the entire reaction is dissolved intothe seawater in this step. Flue gas was sparged until the pH no longerresponded to flue gas dissolution which took approximately 30-60minutes. Agitation was stopped to allow unreacted Moss Mag, sand orother large particles to gravity settle before transferring the CO₂charged acidic water from the first reactor to the second reactor.

The CO₂ charged acidic water was then transferred from the first reactorto the second reactor. The second reactor was used for both nucleationsite generation and crystal growth. After transferring the solution fromthe first reactor to the second reactor, the following steps wereperformed:

-   -   1. 50% NaOH was added until a pH of 9.5 was reached. For        example, for a 1000 gallon reaction, about 20-25 kg of 50% NaOH        was added using a dosing pump capable of pumping 5-25 ml/sec of        50% NaOH. After reaching a pH of 9.5, the addition of 50% NaOH        was stopped.    -   2. A CO₂ source including a mixture of 20% CO₂/80% compressed        air was sparged into the second reactor until a pH of 8.5 was        reached. After reaching a pH of 8.5, the sparging of the CO₂ was        stopped.    -   3. Alternating steps of adding 50% NaOH into the reactor to        raise the pH and sparging CO₂ to lower the pH were performed.        The pH was maintained between 8.5-9.8 during the alternate        addition of the 50% NaOH and sparging of CO₂. Alternate dosing        of 50% NaOH and sparging of CO₂ was continued until a total of        90 kg (i.e., 65-70 kg in this step+20-25 kg from the first step)        of 50% NaOH was added to the reactor.    -   4. The final pH after the last addition of 50% NaOH was between        9.6-9.8    -   5. Agitation was stopped and the precipitate was allowed to        gravity settle overnight and then water/solids separation was        performed. Alternatively, after agitation was stopped, the        precipitate was allowed to gravity settle for 15 minutes and        then accelerated water/solids separation was performed.        Precipitate was maintained at a temperature below 50° C.

Resulting yields ranged from 30-50 lbs of precipitate per 1000 gallonreactor and depended on Mg ion dissolution and total hardness prior toprecipitation.

Example IV CO₂ Absorption

A. Process 1

In this example, absorption of carbon dioxide on the laboratory-scale isdescribed. 4.00 L of seawater was magnetically stirred while 100% CO₂was heavily sparged through the solution for 19 minutes where the pHreached a minimum of 4.89. To this solution, 32.00 g of jet milledMg(OH)₂ was added over a period of 2 minutes. Simultaneously, CO₂ wascontinuously added for a total of 18 minutes to maintain a pH between7.90 and 8.00 as Mg(OH)₂ dissolved. Next, 100.00 mL of 2 M NaOH wasadded over a period of 5 minutes while the pH was maintained between8.00 and 8.10 by addition of CO₂. To facilitate precipitation, 275 mL of2 M NaOH was added over a period of 5 minutes and the resultant solutionwas stirred for an additional 52 minutes. The slurry was vacuum filteredand dried in an oven at 50° C. for 22 hours to recover 19.5 g of calciumand magnesium carbonates (primarily aragonite and nesquehonite,respectively) per 1 L of initial seawater solution.

B. Process 2

In this example, absorption of carbon dioxide on the laboratory-scale isdescribed. A 100-gallon cone-bottomed plastic reaction vessel was filledwith 100 gallons (380 L) of seawater, which was stirred throughout theentire process with an overhead stirrer (Portable Mixer w/Shaft, 2-4″ SSPropeller Blades (1-push, 1-pull), and Mounting Frame). The first stepwas to sparge the solution with CO₂ concentrated at 20% CO₂ and 80%Compressed Air, with a flow rate of 25 scfh. Equilibrium was determinedby the stabilization of the solution pH. The second step was to add 2.70g/L of Mg(OH)₂ (1.02 kg) with heavy mixing. To further facilitate thedissolution of Mg(OH)₂, CO₂ was sparged through the solution. The thirdstep was to add a solution of 50 wt % NaOH until a pH of 9.8 wasreached, followed by additional CO₂ sparging to lower the pH to 8.0.These last two steps of an addition of 50 wt % NaOH to a pH of 9.8 andCO₂ sparging to a pH of 8.0 was repeated until a total of 16.0 kg of 50wt % NaOH had been added to the solution, where the final addition ofNaOH was used to reach a pH of 10.0. The precipitate was separated andcollected from the solution in a yield of 10.24 g/L of calcium carbonateand magnesium carbonate hydrates.

C. Process 3

In this example, absorption of carbon dioxide on the laboratory-scale isdescribed. A 100-gallon cone-bottomed plastic reaction vessel was filledwith 100 gallons (380 L) of seawater, which was stirred throughout theentire process with an overhead stirrer. The first step was to spargethe solution with CO₂ concentrated at 20% by volume at a flow rate of100 scfm (standard cubic feet per minute). Equilibrium was determinedwhen the concentration of CO₂ in the vessel headspace approached that ofthe inlet gas. The calculated absorption of CO₂ during this step wasunderstandably low. The second step was to slowly add 379 g of Mg(OH)₂to avoid a sharp increase in pH which would favor the undesiredcarbonate precipitation. To further facilitate the dissolution ofMg(OH)₂, CO₂ was sparged through the solution to an end pH of 6.3. Thefinal step was to continuously capture CO₂ in the solution. Over thecourse of 3.5 hours, 4.9 kg of NaOH was added to balance the pH at 7.9while CO₂ was sparged and reacted to form bicarbonate ions. Thecalculated absorption of CO₂ during this step was between 68% and 70%.Results are provided in FIG. 15 which shows the evolution of pH and CO₂absorption (instantaneous and cumulative). Artifacts at point 1 in thepH plot were from removal of the pH probe to add Mg(OH)₂.

D. Process 4

In this example, absorption of carbon dioxide on the industrial-scale isdescribed. A 1000-gallon reaction vessel was filled with 900 gallons(3400 L) of seawater, which was stirred throughout the entire process.The first step was to load the solution with 3.3 kg Mg(OH)₂, whichincreases both the pH and the magnesium content. Next, 10% by volume CO₂was sparged and the pH of 7.9 was maintained by a continuous addition ofNaOH up to 30 kg. The total duration of these steps was 5-6 hours. Afinal charge of 38 kg NaOH was added to increase the pH so thatcarbonates would form and precipitate. The duration of this step was10-20 minutes. The solution was stirred for 1 hour more to allow furtherprecipitation. The reaction was allowed to settle overnight. Thesolution was decanted and the solid product was recovered by eitherfilter press or vacuum filtration. Additionally, the solution could berinsed after the decant process; whereby water was added and the samplewas filter pressed. Alternatively, water was added after initial vacuumfiltration, stirred, and filtered again. Finally, the product was spraydried. The overall yield was 5-7 g/L of the original solution.

Example V High Yield Dissolution of Mafic Mineral in HCl

In this example, the dissolution of olivine and subsequent use toprecipitate CO₂ is described. A solution of 10% HCl (475.66 g) was usedto dissolve olivine (10.01 g, particle size ˜5.8 μm) at 50° C. After thesolution was stirred for 10 hours and allowed to sit for 9 hours toprovide a Mg²⁺ _((aq)) concentration of 0.2491 mol/L, it was vacuumfiltered hot to recover 404.52 g filtrate. Over the period of 1 hour,15.01 g NaOH_((s)) and 5.23 g NaOH_((aq)) (in a 50 wt % solution) wereused to neutralize the solution. Simultaneously, 100% CO₂ was heavilysparged through the mixture to provide a final pH of 8.9 whereprecipitate formed. The slurry was vacuum filtered and dried at 50° C.for 17 hours to yield 19.26 g which contained MgCO₃.H₂O, NaCl, anFe-based compound and a Si-based compound.

Example VI Electrochemistry

Exemplary results achieved in accordance with the present bi-electrodesystem are summarized in Table 8 below.

TABLE 8 Low Energy Electrochemical Bi-electrode Method and System Vacross Time Initial pH End pH at Initial pH at End pH at Electrodes(min) at Anode Anode Cathode Cathode 0.45 V 30 4.994 5.204 7.801 7.4310.30 V in the 1^(st), and 0.15 V in the 2^(nd) compartment

In this example, an electrochemistry system for de-protonating seawaterthat has been charged with CO₂ is described. The cell that was usedconsisted of two 1-liter compartments separated by a palladium foil. Thefirst compartment was charged with CO₂ until a pH of 4.994 was achieved.A sacrificial tin anode was placed into the first compartment, and thetin electrode and palladium membrane were held under galvanostaticcontrol at 100nA/cm², which represented a voltage of 0.30V. The secondcompartment consisted of a tin electrode and SnCl₂ dissolved inseawater. The palladium membrane and tin electrode in the secondcompartment where held at 0.15V. The system was run for 30 minutes andas set forth in Table 8, the system showed an increase in pH in thefirst electrolyte, and a decrease in pH in the second electrolyte.

Exemplary results achieved in accordance with the present ionic membranesystem are summarized in Table 9 below.

TABLE 9 Low Energy Electrochemical Ion Exchange System and Method Voltacross Time Initial pH at End pH at Initial pH at End pH at Electrodes(sec) Anode Anode Cathode Cathode 0.6 V 2000 6.7 3.8 6.8 10.8 1.0 V 20006.6 3.5 6.8 11.1

In this example, an electrochemical cell for producing NaOH and HCl at alow operating voltage utilizing an ion exchange membrane positionedbetween an anode and a cathode is described. The cell that was usedconsisted of two 250 mL compartments that were separated by an anionicexchange membrane (PC-SA-250-250 (PCT GmbH of Germany)). In bothcompartments 0.5M NaCl in a 18 MΩ aqueous solution was used. Both theanode and cathode were constructed from a 10 cm×5 cm, 45 mesh Pt gauze.The anode compartment had H₂ gas sparged under the Pt electrode, and thetwo electrodes were held at a bias of 0.6 V and 1.0 V for 2000 seconds.As set forth in Table 9, the two tests achieved a significant increasein the pH in the cathode compartment, and a decrease pH in the anodecompartment.

Although the foregoing invention has been described in some detail byway of illustration and example for purposes of clarity ofunderstanding, it is readily apparent to those of ordinary skill in theart in light of the teachings of this invention that certain changes andmodifications may be made thereto without departing from the spirit orscope of the appended claims.

Accordingly, the preceding merely illustrates the principles of theinvention. It will be appreciated that those skilled in the art will beable to devise various arrangements which, although not explicitlydescribed or shown herein, embody the principles of the invention andare included within its spirit and scope. Furthermore, all examples andconditional language recited herein are principally intended to aid thereader in understanding the principles of the invention and the conceptscontributed by the inventors to furthering the art, and are to beconstrued as being without limitation to such specifically recitedexamples and conditions. Moreover, all statements herein recitingprinciples, aspects, and embodiments of the invention as well asspecific examples thereof, are intended to encompass both structural andfunctional equivalents thereof. Additionally, it is intended that suchequivalents include both currently known equivalents and equivalentsdeveloped in the future, i.e., any design features developed thatperform the same function, regardless of structure. The scope of thepresent invention, therefore, is not intended to be limited to theexemplary embodiments shown and described herein. Rather, the scope andspirit of present invention is embodied by the appended claims.

1. A method of sequestering carbon dioxide, the method comprising: (i)contacting an alkaline-earth-metal-ion-containing salt water with CO₂from an industrial waste stream; (ii) removing protons from saidalkaline-earth-metal-ion-containing salt water by an electrochemicalprotocol, wherein the electrochemical protocol produces no chlorine gas;(iii) subjecting the alkaline-earth-metal-ion-containing salt water tocarbonate compound precipitation conditions to produce a man-madeprecipitated storage stable carbon dioxide sequestering product; and(iv) disposing of the precipitated storage stable carbon dioxidesequestering product to sequester carbon dioxide.
 2. The methodaccording to claim 1, wherein the alkaline-earth-metal-ion-containingsalt water is neutral or acidic when contacted with the CO₂ from anindustrial waste stream.
 3. The method according to claim 1, wherein thealkaline-earth-metal-ion-containing salt water is basic when contactedwith the CO₂ from an industrial waste stream, and wherein the pH of thesalt water is insufficient to cause precipitation of the storage stablecarbon dioxide sequestering product.
 4. The method according to claim 3,wherein the pH of the salt water is maintained at a substantiallyconstant value during contact with the CO₂ from an industrial wastestream.
 5. The method according to claim 4, wherein the pH of the saltwater is maintained at the substantially constant value by adding a baseto the salt water during contact with the CO₂ from an industrial wastestream.
 6. The method according to claim 4, wherein the pH of the saltwater is electrochemically maintained at the substantially constantvalue.
 7. The method according to claim 1, wherein the electrochemicalprotocol produces no oxygen gas.
 8. The method according to claim 1,wherein the electrochemical protocol comprises applying a voltage acrossan anode and a cathode, and produces no gas at the anode.
 9. The methodaccording to claim 8, wherein voltage applied across the anode andcathode is less than 2V.
 10. The method according to claim 8, whereinvoltage applied across the anode and cathode is less than 1.5V.
 11. Themethod according to claim 8, wherein the voltage applied across theanode and cathode is less than 1.0V.
 12. The method according to claim1, wherein the precipitation conditions produce 50 g or more of thestorage stable carbon dioxide sequestering product for every liter ofsalt water.
 13. The method according to claim 1, wherein theprecipitation conditions produce 100 g or more of the storage stablecarbon dioxide sequestering product for every liter of salt water. 14.The method according to claim 1, wherein the precipitation conditionsproduce 200 g or more of the storage stable carbon dioxide sequesteringproduct for every liter of salt water.
 15. The method according to claim1, wherein the storage stable carbon dioxide sequestering productcomprises from 5 to 14% (w/w) carbon.
 16. The method according to claim15, wherein the storage stable carbon dioxide sequestering productcomprises from 6 to 12% (w/w) carbon.
 17. The method according to claim1, wherein 10 to 100% of the carbon present in the storage stable carbondioxide sequestering product is from the industrial waste stream. 18.The method according to claim 17, wherein 50 to 100% of the carbonpresent in the storage stable carbon dioxide sequestering product isfrom the industrial waste stream.
 19. The method according to claim 18,wherein 90 to 100% of the carbon present in the storage stable carbondioxide sequestering product is from the industrial waste stream. 20.The method according to claim 19, wherein 95 to 100% of the carbonpresent in the storage stable carbon dioxide sequestering product isfrom the industrial waste stream.
 21. The method according to claim 1,wherein the storage stable carbon dioxide sequestering product comprisescarbonates.
 22. The method according to claim 1, wherein the carbonatesare magnesium carbonates and calcium carbonates.
 23. The methodaccording to claim 22, wherein the weight ratio of magnesium to calciumcarbonates in the product ranges from 2-3/1.
 24. The method according toclaim 1, wherein the industrial waste stream is a gaseous waste streamproduced by one of a power plant, a foundry, a cement plant, a refinery,and a smelter.
 25. The method according to claim 24, wherein theindustrial gaseous waste stream is power plant flue gas produced bycombustion of a fossil fuel.
 26. The method according to claim 25,wherein the method removes 5% or more of the carbon dioxide from theflue gas with a parasitic energy requirement of 50% or less.
 27. Themethod according to claim 26, wherein the method removes 10% or more ofthe carbon dioxide from the flue gas with a parasitic energy requirementof 30% or less.
 28. The method according to claim 27, wherein the methodremoves 25% or more of the carbon dioxide from the flue gas with aparasitic energy requirement of 25% or less.
 29. The method according toclaim 25, wherein the gaseous waste stream comprises one or more of NOx,SOx, VOC, mercury and particulates and the method results in fixation ofone or more of the NOx, SOx, VOC, mercury and particulates in theprecipitated storage stable carbon dioxide sequestering product.
 30. Themethod according to claim 1, wherein thealkaline-earth-metal-ion-containing salt water comprises calcium andmagnesium.
 31. The method according to claim 30, wherein the salt watercomprises brackish water, sea water, or brine.
 32. The method accordingto claim 30, wherein the method comprises producing thealkaline-earth-metal-ion containing salt water by contacting a precursorwater with a source of calcium ions and magnesium ions.
 33. The methodaccording to claim 1, wherein the disposing comprises placing theproduct at a disposal location.
 34. The method according to claim 1,wherein the disposing comprises employing the product as a component ofa manufactured composition.
 35. The method according to claim 34,wherein the manufactured composition is a building material.
 36. Themethod according to claim 35, wherein the building material is acomponent of concrete.
 37. The method according to claim 36, wherein thecomponent of concrete is chosen from cement, aggregate and supplementarycementitious material.
 38. The method according to claim 37, wherein thebuilding material is a preformed building material.
 39. The methodaccording to claim 34, wherein the manufactured composition is anon-cementitious composition.